QUESTIONSHEETS ACID - BASE EQUILIBRIA. ph OF STRONG ACIDS AND BASES. AND pk a. ph OF ACID OR BASE SOLUTIONS. ph OF MIXED SOLUTIONS OF ACID AND BASE
|
|
- Julian Watts
- 6 years ago
- Views:
Transcription
1 CHEMISTRY QUESTIONSHEETS A2 Level A2 TOPIC 19 ACID - BASE EQUILIBRIA Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet 9 Questionsheet 10 Questionsheet 11 Questionsheet 12 Questionsheet 13 ph and K w ph OF STRONG ACIDS AND BASES STRENGTHS OF ACIDS (K a AND pk a ) ph OF ACID OR BASE SOLUTIONS ph OF MIXED SOLUTIONS OF ACID AND BASE BRØNSTED-LOWRY THEORY I THEORY OF INDICATORS TITRATION CURVES ACID-BASE STRENGTH AND ENTHALPY OF NEUTRALISATION BUFFER SOLUTIONS ph OF BUFFER SOLUTIONS TEST QUESTION I TEST QUESTION II 17 marks 15 marks 14 marks 19 marks 14 marks 15 marks 16 marks 16 marks 15 marks 19 marks 13 marks 16 marks 14 marks Authors Trevor Birt Donald E Caddy Andrew Jones Adrian Bond Editors John Brockington Stuart Barker John Brockington Kevin Frobisher Andy Shepherd Stuart Barker Curriculum Press Licence Agreement: Paper copies of the A-Level Chemistry Questionsheets may be copied free of charge by teaching staff or students for use within their school, provided the Photocopy Masters have been purchased by their school. No part of these Questionsheets may be reproduced or transmitted, in any other form or by any other means, without the prior permission of the publisher. All rights are reserved. This license agreement is covered by the laws of England and Wales Curriculum Press March Curriculum P ress Curriculum Press Bank House 105 King Street Wellington Shropshire TF1 1NU
2 a) Define the term ph. TOPIC 19 Questionsheet 1 ph and K w b) What is meant by the self-ionisation of water? Write an expression for the dissociation constant, and explain how it can be modified so as to define the ionic product (K w ) of water.... [4] c) K w has a numerical value of 1.00 x at 298 K. What are its units? d) At 373 K, K w has a numerical value of 5.14 x Calculate: (i) the concentration of hydrogen ions, [H + ]. the ph of water at this temperature. e) Is the dissociation of water endothermic or exothermic? Justify your answer by reference to the given values of K w.... [4] f) At 273 K, the ph of water is (i) Calculate K w at this temperature. Is water chemically neutral at this temperature? Explain your answer. TOTAL / 17
3 TOPIC 19 Questionsheet 2 ph OF STRONG ACIDS AND BASES a) Calculate the ph of the following solutions (i) mol dm -3 HNO mol dm -3 HCl (iii) mol dm -3 H 2 SO 4 (iv) mol dm -3 KOH (v) mol dm -3 Ba(OH) 2 b) An aqueous solution contains mol of HCl in 100 cm 3 of solution, hence calculate (i) the [H + ] the ph. c) What is the concentration in mol dm -3 of: (i) HCl(aq) which has a ph of 1.4? H 2 SO 4 (aq) which has a ph of 2.7? (iii) NaOH(aq) which has a ph of 11.3? TOTAL / 15
4 TOPIC 19 Questionsheet 3 PH astrengths OF ACIDS (K a AND pk a )nd pk w a) Propanoic acid, C 2 H 5 COOH, is a weak acid, with K a = 1.35 x 10-5 mol dm -3. (i) What is meant by the term weak acid? Write an expression for the acid dissociation constant, K a, of propanoic acid. (iii) Calculate the hydrogen ion concentration and ph of a solution of propanoic acid containing 0.20 mol dm -3. State what assumption is made in the calculation.... [4] b) Two acids, HS and HT, have pk a values of 3.6 and 4.1 respectively. (i) What is meant by the expression pk a? Calculate K a for HS and HT. HS... HT... [2] (iii) Which is the stronger of the two acids? Give your reason. c) The ammonium ion, NH 4+, can act as an acid. (i) Write an expression for the acid dissociation constant, K a, of the ammonium ion. [1] This K a has a value of 5.62 x mol dm -3. Calculate pk a. [1] d) Name of acid Formula pk a Butanoic CH 3 COOH Chlorobutanoic CH 3 CHClCOOH Chlorobutanoic CH 3 CHCl COOH Chlorobutanoic Cl COOH 4.52 Place these acids in order of increasing acid strength. TOTAL / 14
5 TOPIC 19 Questionsheet 4 ph OF ACID OR BASE SOLUTIONSK w a) Calculate the ph of each of the following acids and explain the difference in the values you obtain. (i) mol dm -3 nitric acid mol dm -3 butanoic acid (pk a = 4.82)... [4] Explanation... b) Calculate the ph of the resulting solutions when: (i) 10.0 cm 3 of l.0 mol dm -3 HCl are added to 990 cm 3 of water cm mol dm -3 NaOH are added to 980 cm 3 of water. c) (i) Write an expression for the acid dissociation constant, K a, of methanoic acid, HCOOH. The ph of a solution of methanoic acid, K a = 1.78 x 10-4 mol dm -3, is 4.0. Calculate the concentration of the acid. d) When mol of a weak acid HQ is dissolved in 500 cm 3 of water, the resultant ph is 3.0. Calculate the K a of the acid. TOTAL / 19 [1]
6 TOPIC 19 Questionsheet 5 ph OF MIXED SOLUTIONS OF ACID AND BASE a) Calculate the hydrogen ion concentration in each of the following solutions: (i) mol dm -3 HCl mol dm -3 ethanoic acid (pk a = 4.76). (iii) 100 cm 3 of 0.1 mol dm -3 HCl to which 50 cm 3 of mol dm -3 KOH have been added.... [4] b) Sulfuric acid is a strong dibasic acid, and reacts with potassium hydroxide solution as follows: H 2 SO 4 (aq) + 2KOH(aq) K 2 SO 4 (aq) + 2H 2 O(l) 20.0 cm 3 of sodium hydroxide solution of concentration mol dm -3 were added to 25.0 cm 3 of sulfuric acid of concentration mol dm -3. Calculate: (i) the moles of H + in the sulfuric acid. the moles of OH - added. (iii) the moles of H + unreacted. (iv) the ph of the resulting solution. TOTAL / 14
7 TOPIC 19 Questionsheet 6 BRØNSTED-LOWRY THEORY I a) (i) How does the BrØnsted-Lowry theory define an acid and a base? Acid... Base... [2] What do you understand by the terms conjugate acid and conjugate base? Conjugate acid... Conjugate base... [2] Quality of language [1] b) In each of the following reactions, identify the reacting species which is acting as an acid, and the product species which is the conjugate acid. Acid Conjugate acid (i) CH 3 COOH(aq) + NaOH(aq) CH 3 COONa(aq) + H 2 O(1) HNO 3 (1) + H 2 SO 4 (1) H 2 NO 3+ (aq) + HSO 4 - (aq) (iii) NaHSO 4 (aq) + NaOH(aq) Na 2 SO 4 (aq) + H 2 O (l) [3] c) When dissolved in water, ethylamine, CH 3 NH 2, reacts as follows: CH 3 NH 2 (aq) + H 2 O(1) ¾ CH 3 NH 3+ (aq) + OH - (aq) (i) Explain why ethylamine is regarded as a BrØnsted-Lowry base. Identify the species in the above equation which is the conjugate acid. d) Write equations to show how the hydrogensulfate ion, HSO 4 -, can act as both an acid and a base in aqueous solution. e) Concentrated phosphoric acid reacts with bromide ions as follows: H 3 PO 4 (aq) + Br - (s) ¾ HBr(g) + H 2 PO 4- (aq) Identify the base and the conjugate base in this reaction. Base... Conjugate base... [2] TOTAL / 15
8 TOPIC 19 Questionsheet 7 THEORY OF INDICATORS a) Give three features that a substance must possess if it is to be suitable as an acid-base indicator. b) Acid-base indicators are normally regarded as weak acids, which may be represented by the formula HIn (where In - is the indicator anion). (i) Write an equation for the dissociation in water of an indicator HIn, and hence derive an expression for its indicator constant, K in. [2] What is meant by the term working range of an indicator? (iii) An indicator has a pk in of 5.0; over what ph range would you expect it to change colour? c) The pk in values for three indicators are given below: methyl orange 3.7 bromothymol blue 7.0 thymolphthalein 9.7 State, with reasons, which of these you would choose for a titration of: (i) ethanoic acid (pk a = 4.76) with potassium hydroxide. hydrochloric acid with ethylamine (pk a = 10.7). (iii) ethanoic acid with ethylamine. TOTAL / 16
9 TITRATION CURVES a) The acid dissociation constant, K a, for propanoic acid is 1.35 x 10-5 mol dm -3. Sketch as accurately as possible on the axes below the ph titration curve you would expect to obtain when 20.0 cm 3 of a solution of propanoic acid, containing 0.1 mol dm -3, is titrated with a solution of sodium hydroxide of the same concentration. Show on your graph the initial ph of the acid, the volume of sodium hydroxide used at the end-point, and the ph at the half-equivalence point. 14 TOPIC 19 Questionsheet 8 ph 0 0 Volume NaOH added 40 [5] b) When 25.0 cm 3 of a weak organic acid HA were titrated with 0.2 M sodium hydroxide solution, 18.0 cm 3 of the latter were required for neutralisation. In a subsequent experiment, 9.0 cm 3 of alkali were added to 25.0 cm 3 of the acid; the ph of the resulting solution was Calculate: (i) the concentration of the acid in mol dm -3. the acid dissociation constant, K a. (iii) the ph of the original acid solution. c) On the following axes, sketch the ph titration curves you would expect to obtain for the titration of: (i) 0.1 M NaOH and 0.1 M NH 3 (aq) (pk a = 9.25) with 0.1 M HNO 3. On your sketch, indicate the region over which the ammonia-nitric acid mixture would act as a buffer. 14 ph 0 0 Volume 0.1 M HNO 3 added [5] TOTAL / 16
10 TOPIC 19 Questionsheet 9 ACID-BASE STRENGTH AND ENTHALPY OF NEUTRALISATION a) (i) Define enthalpy of neutralisation. When sulfuric acid is neutralised by sodium hydroxide solution, the enthalpy of neutralisation is -57 kj mol -1 ; the value for the neutralisation of ethanoic acid by sodium hydroxide is -54 kj mol -1. Write chemical equations for these two reactions and explain the difference between the two values. Chemical equations Explanation of difference... b) An experiment to determine the enthalpy of neutralisation of sodium hydroxide with hydrochloric acid produced a value of kj mol -l ; the temperature rise in this experiment was 10.8 K. A similar experiment performed with hydrocyanic acid and ammonia, in which the concentrations of the solutions and the volumes used were the same as in the previous experiment, produced a temperature rise of 1 K. (i) Estimate the enthalpy of neutralisation of hydrocyanic acid (HCN) by ammonia. Explain the difference between the two values obtained.... [4] (iii) Suggest the result you might expect to obtain if hydrocyanic acid were neutralised with sodium hydroxide solution (assuming similar concentrations and volumes). TOTAL / 15
11 TOPIC 19 Questionsheet 10 BUFFER SOLUTIONS a) (i) What do you understand by the term buffer solution? Give one example each of an acid buffer, an alkaline buffer, and a buffer in a biological system. An acid buffer... [1] An alkaline buffer... [1] A buffer in a biological system... [1] b) (i) What do you understand by the expression buffering capacity of a buffer solution? State two factors that will affect the buffering capacity of such a solution. c) (i) Write ionic equations to show how a buffer solution containing ethanoic acid and sodium ethanoate reacts with added H + and OH - ions. Reaction with H + ions... [1] Reaction with OH - ions... [1] The amino acid glycine, H 2 N COOH, is most effective as a buffer at ph values of about 2.3 and 9.6. Assuming that glycine exists as zwitterions rather than molecules, write down the formulae of all organic species present at ph 2.3 and write equations to show how added H + and OH - ions would be removed at this ph. Species present... [2] Reaction with H + ions... [1] Reaction with OH - ions... [1] d) By reference to your knowledge of buffer solutions, explain why, when ethanoic acid is titrated with sodium hydroxide solution, the ph at first changes sharply, and then remains almost unchanged until the end-point of the titration is approached.... [5] TOTAL / 19
12 TOPIC 19 Questionsheet 11 ph OF BUFFER SOLUTIONS a) Calculate the ph of an aqueous solution containing: (i) mol dm -3 ethanoic acid (CH 3 CO 2 H) and mol dm -3 sodium ethanoate. K a for ethanoic acid is mol dm mol dm -3 of bromoethanoic acid (Br CO 2 H) and mol dm -3 sodium bromoethanoate. K a for bromoethanoic acid is mol dm -3 (iii) mol dm -3 of bromoethanoic acid (Br CO 2 H) and mol dm -3 sodium bromoethanoate. K a for bromoethanoic acid is mol dm -3 b) Propanoic acid behaves as a weak acid: CH 3 COOH(aq) ¾ CH 3 COO - (aq) + H + (aq) (i) Write an expression for the acid dissociation constant, Ka, for propanoic acid. A buffer solution of ph 5.0 was prepared by mixing equal volumes of propanoic acid and mol dm -3 sodium propanoate, CH 3 COO-Na +. Calculate the concentration of propanoic acid used to produce this buffer solution. (pka for propanoic acid is 4.87)... [5] [1] TOTAL / 13
13 TOPIC 19 Questionsheet 12 TEST QUESTION I a) A compound was found on analysis to contain: S 26.89% O 13.45% Cl 59.66% Determine its empirical formula. b) 0.05 mol of this compound was dissolved in water and the solution made up to 1.0 dm cm 3 of this solution required 25.0 cm 3 of 0.1 M silver nitrate solution to complete the precipitation of chloride ions. Calculate the number of moles of chloride ions precipitated, and hence determine the molecular formula of the compound. c) A second 25.0 cm 3 portion of the solution was exactly neutralised by sodium hydroxide solution. This neutralised solution, on treatment with excess barium chloride solution, produced g of a white precipitate; this precipitate dissolved in acid, releasing sulfur dioxide. Identify the white precipitate. Given that the compound reacts with water to form a strong monobasic acid HP, and a weak dibasic acid HQ but no other products, identify HP and HQ and write an equation for the reaction of the compound with water.... [6] d) The ph of the solution was measured and found to be (i) Calculate the hydrogen ion concentration in the solution. How many moles of hydrogen ions are produced by the dissociation of 0.05 mol of the weak acid, HQ? (iii) Assuming that the second dissociation of the weak acid can be ignored, calculate the percentage of the total hydrogen ion concentration which is attributable to the weak acid. TOTAL / 16
14 TOPIC 19 Questionsheet 13 TEST QUESTION II In a thermometric titration, 20.0 cm 3 aliquots of a weak acid HZ were titrated individually with 1.0 M sodium hydroxide solution; the maximum temperature rise was recorded for each experiment. The results are given below. Volume 1.0 M NaOH used /cm 3 Maximum temperature rise / C a) Plot these results on the graph paper printed below. [5] TOTAL (Continued...) /
15 TOPIC 19 Questionsheet 13 Continued TEST QUESTION II b) Calculate the concentration of the acid in mol dm -3. c) The ph of the original acid was Calculate K a. d) Determine the enthalpy of neutralisation of this acid by sodium hydroxide. Assume that all solutions have a density of 1.0 g cm -3 and a specific heat capacity of 4.2 J K -1 g -1. TOTAL / 14
TOPIC 19 ANSWERS & MARK SCHEMES QUESTIONSHEET 1. ph AND K W
QUESTIONSHEET 1 a) ph - lg [H + ] / lg 1 [H + ] b) Water ionises slightly as follows: H 2 O(l) ž H + (aq) + OH - (aq) [H + (aq)][oh - (aq)] K c [H 2 O(l)] Since the ionisation is very slight, we regard
More informationQUESTIONSHEETS ORGANIC REACTION MECHANISMS I FREE RADICAL SUBSTITUTION I FREE RADICAL SUBSTITUTION II ELECTROPHILIC ADDITION TO SYMMETRICAL ALKENES
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 14 ORGANIC REACTION MECHANISMS I Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet
More informationQUESTIONSHEETS ENERGETICS I ENTHALPY OF DISPLACEMENT BOND DISSOCIATION ENTHALPY HESS S LAW AND ENTHALPY DIAGRAMS HESS S LAW WITH CALORIMETRY
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 5 ENERGETICS I Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet 9
More informationD. Ammonia can accept a proton. (Total 1 mark)
1. Which statement explains why ammonia can act as a Lewis base? A. Ammonia can donate a lone pair of electrons. B. Ammonia can accept a lone pair of electrons. C. Ammonia can donate a proton. D. Ammonia
More informationQUESTIONSHEETS PERIODIC TABLE I MELTING POINTS AND BOILING POINTS IONISATION ENERGIES AND ELECTRON AFFINITIES ELECTRONEGATIVITIES AND BONDING
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 9 PERIODIC TABLE I Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
More informationQUESTIONSHEETS GROUPS 1 AND 2 REACTIONS OF THE ELEMENTS WITH WATER REACTIONS OF THE ELEMENTS WITH DILUTE ACIDS
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 10 GROUPS 1 AND 2 Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
More informationQUESTIONSHEETS REACTION KINETICS II MEASUREMENT OF REACTION RATES I MEASUREMENT OF REACTION RATES II FIRST ORDER REACTIONS AND HALF-LIFE TIMES
CHEMISTRY QUESTIONSHEETS A2 TOPIC 20 REACTION KINETICS II Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet 9
More information14-Jul-12 Chemsheets A
www.chemsheets.co.uk 14-Jul-12 Chemsheets A2 009 1 BRONSTED-LOWRY ACIDS & BASES Bronsted-Lowry acid = proton donor (H + = proton) Bronsted-Lowry base = proton acceptor (H + = proton) Bronsted-Lowry acid-base
More information, for C 2. COOH is mol dm [1] COOH by adding water until the total volume is cm 3. for C 2 COOH.
1 A student is supplied with 0.500 mol dm 3 potassium hydroxide, KOH, and 0.480 mol dm 3 propanoic acid, C 2 COOH. The acid dissociation constant, K a, for C 2 COOH is 1.35 10 5 mol dm 3. (a) C 2 COOH
More information(14) WMP/Jun10/CHEM4
Acids, Bases and ph 14 5 In this question, give all values of ph to two decimal places. Calculating the ph of aqueous solutions can involve the use of equilibrium constants such as K w and K a K w is the
More information12. Acid Base Equilibria
2. Acid Base Equilibria BronstedLowry Definition of acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that can
More informationQUESTIONSHEETS ACID-BASE TITRATIONS PREPARATION OF A STANDARD SOLUTION SIMPLE VOLUMETRIC CALCULATIONS
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 3 ACID-BASE TITRATIONS Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
More informationANSWERS Unit 14: Review Acids and Bases
ANSWERS Unit 14: Review Acids and Bases 1) CH 3 COOH(aq) + H 2 0(l) H 3 0 + (aq) + CH 3 COO - (aq) In the equilibrium above, what are the two conjugate bases? A. CH 3 COOH and H 2 0 B. CH 3 COO - and H
More information1.12 Acid Base Equilibria
.2 Acid Base Equilibria BronstedLowry Definition of acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that can
More informationChemical Equilibria Part 2
Unit 1 - Inorganic & Physical Chemistry 1.4 Chemical Equilibria Part 2 Acid / Base Equilibria Indicators ph Curves Buffer Solutions Pupil Notes Learning Outcomes Questions & Answers KHS ChemistrySept 2015
More informationWrite the ionic equation for this neutralisation reaction. Include state symbols.
Q1.Sodium hydroxide neutralises sulfuric acid. The equation for the reaction is: 2NaOH + H 2 SO 4 Na 2 SO 4 + 2H 2 O (a) Sulfuric acid is a strong acid. What is meant by a strong acid? (b) Write the ionic
More information5.1.3 Acids, Bases and Buffers
5..3 Acids, Bases and Buffers BronstedLowry Definition of Acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that
More informationTitration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below.
Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below. All solutions have concentrations of 0. mol dm 3. (a) In this part of the question,
More informationQUESTIONSHEETS ENERGETICS II ENTHALPY OF ATOMISATION ENTROPY AND FREE ENERGY CHANGE PRINCIPLES OF ELECTROCHEMICAL CELLS
CHEMISTRY QUESTIONSHEETS A2 Level A2 TOPIC 17 ENERGETICS II Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
More information4. Acid Base Equilibria
4. Acid Base Equilibria BronstedLowry Definition of acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that can
More informationOCR (A) Chemistry A-level Topic Acids, Bases and Buffers
OCR (A) Chemistry A-level Topic 5.1.3 - Acids, Bases and Buffers Flashcards Define a Bronsted-Lowry acid Define a Bronsted-Lowry acid Proton donor Define a Bronsted-Lowry base Define a Bronsted-Lowry base
More informationmohd faisol mansor/chemistry form 4/chapter 7 CHAPTER 7 ACIDS AND BASES HCl (g) H 2 O H + (aq) + Cl - (aq) NaOH(s) H 2 O Na + (aq) + OH - (aq)
CHAPTER 7 ACIDS AND BASES Arrhenius Theory An acid is a chemical compound that produces hydrogen ions, H + or hydroxonium ions H3O + when dissolve in water. A base defined as a chemical substance that
More information4.3 ANSWERS TO EXAM QUESTIONS
4. ANSWERS TO EXAM QUESTIONS. (a) (i) A proton donor () (ii) Fully ionised or fully dissociated () (iii) 0 0 4 () mol dm 6 () 4 (b) (i) 50 0 /5 000 () = 0 06 mol dm () () (ii) Mol OH added = 50 0 50/000
More information+ H 2 O HPO 4. (a) In this system, there are two acid-base conjugate pairs. These are (1) HPO4
1 The dihydrogenphosphate-hydrogenphosphate ion system is an important buffer in the human body. H 2 PO 4 H 2 O HPO 4 2 H 3 O (a) In this system, there are two acid-base conjugate pairs. These are acid
More informationA2 LEVEL CHEMISTRY ACIDS, BASES AND BUFFERS TEST
A2 LEVEL CHEMISTRY 5.1.3 ACIDS, BASES AND BUFFERS TEST Answer all questions Max 50 marks Name.. Mark../50...% Grade Paddington Academy 1 1. A student carried out an investigation with aqueous solutions
More informationGrade A buffer: is a solution that resists changes in its ph upon small additions of acid or base.sq1
Chapter 15 Lesson Plan Grade 12 402. The presence of a common ion decreases the dissociation. BQ1 Calculate the ph of 0.10M CH 3 COOH. Ka = 1.8 10-5. [H + ] = = ( )( ) = 1.34 10-3 M ph = 2.87 Calculate
More informationph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor
ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate
More informationQUESTIONSHEETS STRUCTURE AND BONDING SHAPES OF MOLECULES AND IONS I SHAPES OF MOLECULES AND IONS II IONIC BONDING TENDING TOWARDS COVALENCY
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 4 STRUCTURE AND BONDING Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
More informationStrong & Weak Acid (ph, pka, Kw) Question Paper
For more awesome GSE and level resources, visit us at www.savemyexams.co.uk/ Strong & Weak cid (ph, pka, Kw) Question Paper Level Subject Exam oard Topic Sub Topic ooklet Paper Type Level hemistry Edexcel
More information( 1 ) Concept of acid / base
Section 6.2 Ionic Equilibrium Unit 628 ( 1 ) Concept of acid / base The best definition of acids and bases is that proposed by T.M. Lowry and also, independently by J.N. Bronsted in 1923. BronstedLowry
More information5.1 Module 1: Rates, Equilibrium and ph
5.1 Module 1: Rates, Equilibrium and ph 5.1.1 How Fast? The rate of reaction is defined as the change in concentration of a substance in unit time Its usual unit is mol dm 3 s 1 When a graph of concentration
More informationAP Chapter 15 & 16: Acid-Base Equilibria Name
AP Chapter 15 & 16: Acid-Base Equilibria Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 15 & 16: Acid-Base Equilibria 2 Warm-Ups (Show
More information1. Which statement is correct for a crystal of iron(ii) sulfate in a state of equilibrium with a saturated solution of iron(ii) sulfate?
1. Which statement is correct for a crystal of iron(ii) sulfate in a state of equilibrium with a saturated solution of iron(ii) sulfate? A. The colour of the solution darkens as the crystal continues to
More informationChem!stry. Assignment on Acids, Bases and Salts #
Chem!stry Name: ( ) Class: Date: / / Assignment on Acids, Bases and Salts #5 Write your answers in the spaces below: 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 1. Which of the
More informationcm mol l -1 NaOH added to 50.0 cm 3 of 0.10 mol l -1 HCl
cm 3 0.10 mol l -1 NaOH added to 50.0 cm 3 of 0.10 mol l -1 HCl Acids have been described as substances that dissolve in water to form H + (aq) ions, whilst bases are substances that react with acids.
More informationEdexcel Chemistry A-level Topic 12 - Acid-Base Equilibria
Edexcel Chemistry A-level Topic 12 - Acid-Base Equilibria Flashcards Define a Bronsted-Lowry acid Define a Bronsted-Lowry acid Proton donor Define a Bronsted-Lowry base Define a Bronsted-Lowry base Proton
More informationLesmahagow High School AHChemistry Inorganic and Physical Chemistry Lesmahagow High School CfE Advanced Higher Chemistry
Lesmahagow High School CfE Advanced Higher Chemistry Unit 1 Inorganic and Physical Chemistry Chemical Equilibrium 1 Dynamic Equilibrium Revision Dynamic equilibrium happens in a closed system when the
More informationAcids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set
Acids, Bases, & Neutralization Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Acids, Bases, & Neutralization 2 Study Guide: Things You Must Know
More informationT8-1P1 [212 marks] [1 mark] Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2.
T8-1P1 [212 marks] 1. Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2 2. Which of the following is correct? A. A weak acid is a proton donor and
More informationGrace King High School Chemistry Test Review
CHAPTER 19 Acids, Bases & Salts 1. ACIDS Grace King High School Chemistry Test Review UNITS 7 SOLUTIONS &ACIDS & BASES Arrhenius definition of Acid: Contain Hydrogen and produce Hydrogen ion (aka proton),
More informationNo Brain Too Small CHEMISTRY AS90700 Describe properties of aqueous systems. ph of weak acids, weak bases and salt solutions
ph of weak acids, weak bases and salt solutions 2010: 1 An aqueous solution of ammonium chloride (NH 4 Cl) has a ph of 4.66. (a) (i) Write the equation for solid ammonium chloride dissolving in water.
More informationAims to increases students understanding of: History, nature and practice of chemistry. Applications and uses of chemistry
Aims to increases students understanding of: History, nature and practice of chemistry Applications and uses of chemistry Implications of chemistry for society and the environment 1. Definitions: Lavoisier
More information... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3
1 Chemists have developed models for bonding and structure which are used to explain different properties. (a) Ammonia, NH 3, is a covalent compound. Explain what is meant by a covalent bond. Draw a dot-and-cross
More informationNH 3(aq) + H + (aq)
Q1.A solution of chlorine in water is acidic. Swimming pool managers maintain pool water at a constant ph by using a buffer. They do so by adding sodium hydrogencarbonate and sodium carbonate. (a) Hydrogen
More informationmoulsham high school 1
moulsham high school 1 a) Interpret the natural direction of change (spontaneous change) as the direction of increasing number of ways of sharing energy and therefore of increasing entropy (positive entropy
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More informationPHYSICAL SCIENCES: PAPER II
NATIONAL SENIOR CERTIFICATE EXAMINATION NOVEMBER 2014 PHYSICAL SCIENCES: PAPER II Time: 3 hours 200 marks PLEASE READ THE FOLLOWING INSTRUCTIONS CAREFULLY 1. This question paper consists of 14 pages, a
More informationPaper Reference. Tuesday 22 January 2008 Morning Time: 1 hour 30 minutes
Centre No. Candidate No. Paper Reference(s) 6244/01 Edexcel GCE Chemistry Advanced Unit Test 4 Tuesday 22 January 2008 Morning Time: 1 hour 30 minutes Materials required for examination Nil Candidates
More informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
More informationUnit 4: General Principles of Chemistry I Rates, Equilibria and Further Organic Chemistry (including synoptic assessment)
Write your name here Surname Other names Edexcel GCE Centre Number Candidate Number Chemistry Advanced Unit 4: General Principles of Chemistry I Rates, Equilibria and Further Organic Chemistry (including
More informationEquilibrium principles in aqueous systems are limited to qualitative descriptions and/or calculations involving:
NCEA Chemistry 3.6 Aqueous Systems AS 91392 Demonstrate understanding of equilibrium principles in aqueous systems Aqueous systems are limited to those involving sparingly soluble ionic solids Equilibrium
More informationACIDS, BASES & SALTS DR. RUCHIKA YADU
ACIDS, BASES & SALTS DR. RUCHIKA YADU Properties of Acids Acid is a compound which yields hydrogen ion (H+), when dissolved in water. Acid is sour to the taste and corrosive in nature. The ph value of
More informationA level Chemistry Preparation Work
A level Chemistry Preparation Work This booklet is designed to help you prepare for you re A level studies in chemistry. Tasks have been selected to improve your grounding in key skills and concepts that
More information1. An aqueous solution of which of the following reacts with magnesium metal?
1 1. An aqueous solution of which of the following reacts with magnesium metal? A. Ammonia B. Hydrogen chloride C. Potassium hydroxide D. Sodium hydrogencarbonate 2. Which one of the following species
More informationLevel 3 Chemistry Demonstrate understanding of equilibrium principles in aqueous systems
1 SUGGESTED ANSWERS please email any corrections / suggestions Level 3 Chemistry 91392 Demonstrate understanding of equilibrium principles in aqueous systems Credits: Five Achievement Achievement with
More informationPage 2. Q1.Water dissociates slightly according to the equation: H 2 O(I) The ionic product of water, K w, is given by the expression
Q1.Water dissociates slightly according to the equation: H 2 O(I) H + (aq) + OH (aq) The ionic product of water, K w, is given by the expression K w = [H + ][OH ] K w varies with temperature as shown in
More informationSchool of Chemistry, University of KwaZulu-Natal, Howard College Campus, Durban. CHEM191 Tutorial 1: Buffers
School of Chemistry, University of KwaZulu-Natal, Howard College Campus, Durban CHEM191 Tutorial 1: Buffers Preparing a Buffer 1. How many moles of NH 4 Cl must be added to 1.0 L of 0.05 M NH 3 to form
More information1 A. That the reaction is endothermic when proceeding in the left to right direction as written.
1 Q. If Δ r H is positive, what can you say about the reaction? 1 A. That the reaction is endothermic when proceeding in the left to right direction as written. 2 Q If Δ r H is negative, what can you say
More informationPublic Review - Acids and Bases. June A solution of which ph would make red litmus paper turn blue? (A) 2 (B) 4 (C) 6 (D) 8
Public Review Acids and Bases June 2005 13. A solution of which ph would make red litmus paper turn blue? 2 4 6 8 14. Which is the most recent definition of an acid? Arrhenius Brønsted)Lowry modified Arrhenius
More informationAP Chemistry: Acid-Base Chemistry Practice Problems
Name AP Chemistry: Acid-Base Chemistry Practice Problems Date Due Directions: Write your answers to the following questions in the space provided. For problem solving, show all of your work. Make sure
More informationAcids, Bases and Buffers
1 Acids, Bases and Buffers Strong vs weak acids and bases Equilibrium as it relates to acids and bases ph scale: [H+(aq)] to ph, poh, etc ph of weak acids ph of strong acids Conceptual about oxides (for
More information*P51939A0124* Pearson Edexcel WCH04/01. P51939A 2018 Pearson Education Ltd.
Write your name here Surname Other names Pearson Edexcel International Advanced Level Centre Number Candidate Number Chemistry Advanced Unit 4: General Principles of Chemistry I Rates, Equilibria and Further
More informationCHAPTER 7.0: IONIC EQUILIBRIA
Acids and Bases 1 CHAPTER 7.0: IONIC EQUILIBRIA 7.1: Acids and bases Learning outcomes: At the end of this lesson, students should be able to: Define acid and base according to Arrhenius, Bronsted- Lowry
More informationA-level CHEMISTRY 7405/1. Paper 1: Inorganic and Physical Chemistry. SPECIMEN MATERIAL v1.2
SPECIMEN MATERIAL v1.2 Please write clearly in block capitals. Centre number Candidate number Surname Forename(s) Candidate signature A-level CHEMISTRY Paper 1: Inorganic and Physical Chemistry Specimen
More informationArrhenius base is one that dissociates in water to form hydroxide ions.
Chemistry Notes: Acids and Bases Arrhenius base is one that dissociates in water to form hydroxide ions. Arrhenius acid is on that dissociates in water to form hydrogen ions (protons). A Bronsted-Lowry
More informationLevel 2 Chemistry, 2017
91166 911660 2SUPERVISOR S Level 2 Chemistry, 2017 91166 Demonstrate understanding of chemical reactivity 2.00 p.m. Thursday 16 November 2017 Credits: Four Achievement Achievement with Merit Achievement
More informationCOOH, and thioglycolic acid, HSCH 2. (a) Glycolic acid reacts with bases, such as aqueous sodium hydroxide, NaOH(aq), to form salts.
1 Glycolic acid, HOCH 2 COOH, and thioglycolic acid, HSCH 2 COOH, are weak acids. (a) Glycolic acid reacts with bases, such as aqueous sodium hydroxide, NaOH(aq), to form salts. A student pipetted 25.0
More informationThe Acidic Environment
The Acidic Environment HSC ENRICHMENT DAY Artchaki Chandrasegar & Alexander Comerford Key points of the acidic environment TODAY, WE WILL FOCUS ON: 1. Definitions: Lavoisier / Davy; Arrhenius; Brønsted-Lowry;
More information(iii) Use the diagram to determine the value (mol 2 dm 6 ) of K w at 50 C. [1]
2. (a) The diagram shows the variation of the ionic product of water, K w, with temperature. 6 K w /10 14 mol 2 dm 6 Temperature/ C (i) Give the expression for the ionic product of water, K w. [1] (ii)
More informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases Properties of Acids and Bases What is an acid? Some examples of common items containing acids: Vinegar contains acetic acid; lemons and citrus fruits contain citric acid; many
More informationQUESTIONSHEETS LABORATORY CHEMISTRY MELTING POINTS AND BOILING POINTS TESTS FOR FUNCTIONAL GROUPS. ORGANIC TEST QUESTION IV (Using IR Spectra)
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 16 LABORATORY CHEMISTRY Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
More informationK a =
Q1.The acid dissociation constant, K a, for ethanoic acid is given by the expression K a = The value of K a for ethanoic acid is 1.74 10 5 mol dm 3 at 25 C. A buffer solution is prepared using ethanoic
More informationUnit Nine Notes N C U9
Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release
More information2 Answer all the questions.
2 Answer all the questions. 1 Born Haber cycles provide a model that chemists use to determine unknown enthalpy changes from known enthalpy changes. In this question, you will use a Born Haber cycle to
More informationPage 2. Q1.Water dissociates slightly according to the equation: H 2 O(I) The ionic product of water, K w, is given by the expression
Q1.Water dissociates slightly according to the equation: H 2 O(I) H + (aq) + OH (aq) The ionic product of water, K w, is given by the expression K w = [H + ][OH ] K w varies with temperature as shown in
More informationUnit 2 Acids and Bases
Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions
More informationAcids and Bases Written Response
Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink
More informationChemistry Assessment Unit A2 1
Centre Number 71 Candidate Number ADVANCED General Certificate of Education 2014 Chemistry Assessment Unit A2 1 assessing Periodic Trends and Further Organic, Physical and Inorganic Chemistry AC212 [AC212]
More informationIB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.
IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any
More informationName: C4 TITRATIONS. Class: Question Practice. Date: 97 minutes. Time: 96 marks. Marks: GCSE CHEMISTRY ONLY. Comments:
C4 TITRATIONS Question Practice Name: Class: Date: Time: 97 minutes Marks: 96 marks Comments: GCSE CHEMISTRY ONLY Page of 3 Sodium hydroxide neutralises sulfuric acid. The equation for the reaction is:
More informationDescribe the structure and bonding in a metallic element. You should include a labelled diagram in your answer. ... [3] ...
3 Gallium is a metallic element in Group III. It has similar properties to aluminium. (a) (i) Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer.
More informationSIR MICHELANGELO REFALO CENTRE FOR FURTHER STUDIES VICTORIA GOZO
SIR MICHELANGELO REFALO CENTRE FOR FURTHER STUDIES VICTORIA GOZO Page 1 of 7 Half Yearly Exam 2013 Subject: Chemistry 1 st Year Level: Advanced Time: 3 hrs Answer SEVEN (7) questions. All questions carry
More informationComplete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion.
1 This question is about the elements with atomic numbers between 58 and 70 (a) Cerium, atomic number 58, is a metal Complete the table to show the relative charge of each particle and the number of each
More information+(aq) + Cl - (aq) HA(aq) A - (aq) + H + (aq) CH 3COO - (aq) + H + (aq)
1 A2 Chemistry: F325 Equilibria, Energetics and Elements 5.1.3 Acids, Bases and Buffers. Lesson 6 Buffer Solutions. Learning Outcomes: All Describe what is meant by the term buffer solution (5.1.3 k) Explain
More informationACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY
ACIDS AND BASES A. CHARACTERISTICS OF ACIDS AND BASES 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More information2 Answer all the questions. 1 Born Haber cycles can be used to calculate enthalpy changes indirectly.
2 Answer all the questions. 1 Born Haber cycles can be used to calculate enthalpy changes indirectly. (a) The table below shows enthalpy changes for a Born Haber cycle involving potassium sulfide, K 2
More informationAcids and Bases Written Response
Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink
More information9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS
9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS Work directly from Zumdahl (Chapter 4). Work through exercises as required, then summarise the essentials of the section when complete. To understand the
More informationThe characteristic Properties of Acids and
For more awesome GSE and level resources, visit us at www.savemyexams.co.uk/ The haracteristic Properties of cids and ases Question Paper Level Subject Exam oard Topic Sub-Topic ooklet O Level hemistry
More informationChapter 6. Acids, Bases, and Acid-Base Reactions
Chapter 6 Acids, Bases, and Acid-Base Reactions Chapter Map Arrhenius Acid Definition Anacid is a substance that generates hydronium ions, H 3 O + (often described as H + ), when added to water. An acidic
More informationOCR A Chemistry A-Level Module 5 - Physical Chemistry & Transition Elements
OCR A Chemistry A-Level Module 5 - Physical Chemistry & Transition Elements Acids and Bases Notes and Example Calculations Answers given at the end of the booklet ph Acid Calculations Strong Acids To calculate
More informationAP Study Questions
ID: A AP 16.4-16.7 Study Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1 What is the ph of an aqueous solution at 25.0 C in which [H + ] is 0.0025
More information7 Acids and bases. Answers to worked examples
s manual for Burrows et.al. Chemistry 3 Third edition 7 Acids and bases Answers to worked examples WE 7.1 Conjugate acids and conjugate bases (on p. 307 in Chemistry 3 ) Pure ethanoic acid (CH 3 CH 2 OH)
More information2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds
2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds. (a) Define, in words, the term lattice enthalpy............. [2] (b) The Born Haber cycle
More informationTopic 9: Acids & Bases
Topic 9: Acids & Bases Regents Chemistry Mr. Mancuso Electrolytes Substances that conduct electricity when Include Ability to conduct electricity is due to the presence of Dissociation: ~ 1 ~ Acids and
More informationPaper Reference. Advanced Unit Test 6B (Synoptic) Monday 25 June 2007 Morning Time: 1 hour 30 minutes
Centre No. Paper Reference Surname Initial(s) Candidate No. 6 2 4 6 0 2 Signature Paper Reference(s) 6246/02 Edexcel GCE Chemistry Examiner s use only Team Leader s use only Advanced Unit Test 6B (Synoptic)
More informationAcids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY
Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationB410U10-1 S16-B410U10-1. CHEMISTRY Component 1 The Language of Chemistry, Structure of Matter and Simple Reactions
Surname Centre Number Candidate Number Other Names 2 GCE AS NEW AS B410U10-1 S16-B410U10-1 CHEMISTRY Component 1 The Language of Chemistry, Structure of Matter and Simple Reactions A.M. FRIDAY, 27 May
More information