Acids and Bases o Naming o Definitions o Indicators ( ) o ph poh calculations Molarity o Calculations o Dilution Titration

Transcription

1 General Chemistry Unit 13 Acids and Bases o Naming o Definitions o Indicators ( ) o ph poh calculations Molarity o Calculations o Dilution Titration 1

2 How to recognize a compound/formula as being an acid or base: Acid: has H, hydrogen, at the beginning. Base: contains OH, hydroxide. Naming Acids Binary Acids Contain H and one other element To name: hydro + second element(change ending to ic) + acid HCl = Hydro chlorine ic + acid Hydrochloric acid HF = Hydro fluorine ic + acid Hydrofluoric acid HI = H 2 S = *If you are given the name and must write the formula, make sure you check charges and do the criss-cross! Ternary Acids (Polyatomics) Contain H, O and one more element (a polyatomic ion with O in it; SO4) To Name: For ate and per 1. HNO3 = nitric acid (was nitrate) 2. H2SO4 = sulfuric acid (was sulfate) 3. HC2H3O2 = acetic acid (was acetate) (acetate is also CH3COO) 4. H2SO5 = persulfuric acid (was persulfate) 5. H3PO4 = phosphoric acid (was phosphate) 6. HClO3 = 7. HNO 4 = 8. HIO 4 = -ate polyatomic ions, change the ate ending to ic acid. 2

3 -ite and hypo -ite polyatomic ions become ous acid. 1. HNO2 = nitrous acid (was nitrite) 2. HNO = hyponitrous acid (was hyponitrite) 3. H2SO3 = 4. H2SO2 = 5. HClO = 6. HIO= Naming Bases: Name the metal first + hydroxide NaOH = sodium hydroxide Ca(OH) 2 = calcium hydroxide Fe(OH) 3 = iron (III) hydroxide 3

4 Naming Acids and Bases Name the following: 1. HI 2. HClO3 3. Pb(OH)4 4. H3PO4 5. LiOH 6. H2SO3 7. HNO4 8. H2CO 9. Fe(OH)3 10. HCl 11. Ca(OH)2 12. HBrO Write the formula for the following: 13. Percarbonic acid 19. Mercury (II) hydroxide 14. Hydrofluoric acid 20. Acetic acid 15. Chlorous acid 21. Barium hydroxide 16. Hyposulfurous acid 22. Nitrous acid 17. Persulfuric acid 23. Hypophosphorous acid 18. Zinc hydroxide 24. Sulfuric acid 4

5 Names & Formulas of Acids and Bases Chemical Formula Base, Binary acid, or Ternary acid Chemical Name 1. HF 2. HClO3 3. Al(OH)3 4. H2CO3 5. KOH 6. HNO2 7. H2SO4 8. H3PO4 9. Fe(OH)3 10. HClO 11. Ca(OH)2 12. HBr Write the formula for the following: 13. Sulfurous acid 19. Nitrous acid 14. Magnesium hydroxide 20. Iron (II) hydroxide 15. Iodic acid 21. Hydroselenic acid 16. Hydrochloric acid 22. Carbonic acid 17. Hydroiodic acid 23. Acetic acid 18. Perchloric acid 24. Nitric acid 5

6 Acids and Bases Properties of Acids 1. Taste 2. Itchy on skin 3. Blue Litmus turns Red Litmus Stays 4. React with Bases Neutralization: Acid + Base Salt + Water Examples Vinegar Citrus Fruit Properties of Bases 1. Tastes 2. Feels slippery 3. Red Litmus turns Blue Litmus stays 4. React with Acids Neutralization: Acid + Base Salt + Water Examples Soaps Milk of Magnesia Ammonia 6

7 ph Measurement 1. Litmus paper Red for Acid Blue for Base Cheap but very qualitative; only can tell if acid or base 2. Chemical Indicators Color change in a small ph range Many chemical indicators to choose from o Universal Indicator ph 4 to ph 10 Various colors o Phenolphthalein Clear to Magenta at ph = 9 o Natural Indicator Cabbage anthocyanin pigment Get more information as it can be matched to a color to get an approximate ph. Universal Indicator 3. ph Meter most accurate method Get a numerical value Most expensive but get quantitative data. 7

8 Acids and Bases 3 Theories Theory 1 = Traditional (Arrhenius) Acid - Formula has H written first and ionizes in water to form HYDRONIUM ION o Hydronium Ion = H3O + o HF + H2O F - + H3O + Base Formula has OH at end and ionizes in water to form HYDROXIDE ION o Hydroxide Ion = OH - o LiOH Li + + OH - Salt Compound whose chemical formula does not contain H first or OH last o BaSO4 Practice: ( Acid, Base or Salt) 1. H2SO4 2. LiCl 3. HNO3 4. KOH 5. NaNO3 6. Ba(OH)2 8

9 Theory 2 = Bronsted-Lowry Theory Acid a proton donor donates or loses H + Base = proton acceptor accepts H + o Acid and Base are located on left side of arrow (reactant side) Conjugate Acid (conjugate means becoming.more Acid) forms when Base accepts H + Conjugate Base (conjugate means becoming.more Base) piece of Acid left after H + is donated o C. Acid and C. Base are located on right side of arrow (product side) Acid + Base C. Acid + C.Base 1. CH3OH + NH2-1 CH3O +1 + NH3 2. HCN + SO4-2 HSO4-1 + CN CN -1 + HBr HCN + Br HCl + PO4-3 HPO4-2 + Cl HNO3 + H2PO4-1 NO3-1 + H3PO4 9

10 Theory 3 = Lewis Theory Acid electron pair acceptor (no extra lone pair on central atom) Base electron pair donor (an extra electron lone pair on the central atom) o BH3 o PBr3 o SeI4 o SF6 10

11 The ph Scale Measure or count of the hydrogen (hydronium) ion concentration Scale ranges from 0 14 o 7 > = acidic (0 is most acidic) o 7 = neutral o 7 < = basic (14 is most basic) Have Need Equation ph [H + ] 10 -ph poh [OH - ] 10 -poh [H + ] ph -log[h + ] [OH - ] poh -log[oh - ] [H + ] and [H3O + ] are the same ph + poh =14 11

12 Problem #1: ph of.01m HNO3 solution ph = Problem #2: ph of M HC2H3O2 ph = Problem #3: ph of solution with a hydrogen concentration of 2.3 x 10-6 M? ph = Problem #4: poh of.0001 M NaOH poh = Problem #5: ph of.0001 M NaOH Problem #6: ph and poh of M KOH Problem #7: Find [H + ] if poh = 3 12

13 Acid Base Calculation Practice 1. What is the hydroxide ion concentration of a solution whose ph is 12.40? 2. What is the ph of a M NaOH solution? 3. If [H3O +1 ] = 8.26 x 10-5 M, what is the ph of the solution? 4. If the hydroxide concentration is 3.00 x M, what is the hydronium concentration? 5. A substance has an OH - concentration of 5.00 x 10-3 M. What is the ph of this substance? 6. If a solution of acid has a H + concentration of 7.80 x 10-4 M, what is its hydroxide concentration? 13

14 Indicators and ph I. Problem: Many different compounds tend to change color in different types of solutions. Is there a relationship between these colors and the ph of the solutions? Can I use these color changes to predict the ph of an unknown solution? II. Background Information: ph is a unit that has been designed to determine the strength of an acid. This unit is a count of the hydronium ions so that a determination of the acid strength of a solution can be made. Several substances change color with different ph. These color differences can then be used to determine the approximate ph of a substance. III. Procedure: 1) Place a clean and dried microplate on a piece of white paper. 2) Add ~25 drops (about half of the well) of each varying ph solution according to data table 1. (Ex. add vinegar to the four wells in the column labeled vinegar). Also, use an unknown solution in the sixth column and record its letter in table 1. a. Add 2 drops of Bromothymol Blue to each well in the first row. b. Add 2 drops of Universal Indicator to each well in the second row. c. Add 2 drops of Phenolphthalein to each well in the third row. 3) Gently swirl the well plate to mix the solutions completely. 4) Record the resulting colors in the data table. 5) Use the solution in the fourth row (no indicator) to test the ph using the red and blue litmus paper: a. Place one piece each of the red and blue litmus paper on a paper towel. b. Use a clean glass stirring-rod to obtain a tiny droplet of the solution to be tested and apply it to a clean area of the litmus paper. c. Wipe dry the stirring-rod before testing another solution. d. Record your observations in the data table. 6) Use this info to determine the ph value (to the tenth place) of the unknown. ph= 7) Raise your hand so the instructor can use a digital ph meter to test your accuracy. ph meter reading= Data table 1. Vinegar ph=3.0 Seltzer Water ph=5.5 Neutral ph= M NaHCO3 ph=10.0 Ammonia ph=12.0 Unknown Letter Bromothymol Blue Universal Indicator Phenolphthalein Red Litmus Blue Litmus Cabbage Juice 14

15 IV. Data Analysis: 1) At what ph(s) does bromothymol blue, universal indicator, and phenolphthalein change color? bromothymol blue ph of color change universal indicator Phenolphthalein 2) a. What color does red litmus turn in the presence of an acid and a base? b. What color does blue litmus turn in the presence of an acid and a base? 3) Which indicator(s) gives no information in the acid-to-neutral ph range? 4) Calculate the hydronium concentration of the unknown solution using the estimated ph value and the ph meter reading. (Remember ph = - log [H3O + ], or 10 -ph = [H3O + ]) [H3O + ] from estimated ph value [H3O + ] from ph meter reading 15

16 Review for Acids and Bases 1. Based on Arrhenius s definition of acid, base and salt, predict which of the following compounds are acids, bases or salts. Ca3(PO4)2 HBr Cr(OH)2 HgCl2 H2Se 2. Based on the Bronsted-Lowry Theory of acids and bases, predict where a hydrogen is being lost, where it is being gained, and label the reactants and products: a. HCl + NH3 NH4 + + Cl - b. SO H2O HSO4 - + OH - 3. For these compounds, predict if they are a Lewis acid or Lewis base.i need to see the dots! a. PF5 b. NBr3 4. Are the following acids: binary or ternary? Acid Binary or Ternary H2SO4 HBr H2CO3 HI H2Se 16

17 5. Fill in the Table: Chemical Formula H2Se HBrO HCl Ba(OH)2 HClO2 Name Iron (III) hydroxide Phosphoric Acid Nitrous acid Sulfuric acid Iodic acid Hydroiodic acid 6. How many color changes do most chemical indicators go through between a ph of 0 and a ph of 14? 7. What is the indicator that we used that is very unique in that it changes color 7 times between a ph of 4 and a ph of 10? 8. True or False: Cabbage Juice only goes through 1 color change between 0 and 14? 9. When using litmus paper, acid is represented by what color? 10. When using litmus paper, base is represented by what color? 11. List 3 properties of acids and 3 properties of bases. 12. What is the ph of a M HCl solution? 13. What is the poh of a M HCl solution? 14. What is the concentration of [OH - ] if the ph is 5.84? 17

18 1. Solution Solution Terms 2. Solvent 3. Solute 4. Aqueous solution 5. Concentrated 6. Dilute 7. Molarity (M) 8. Dilution Process in Chemistry 18

19 Molarity Measure of the strength of a solution Strong has molarity Weak has molarity Solution has 2 parts o what gets mixed in o what does the dissolving (typically water) Quantitative need accuracy Typically use volumetric flasks Include Molarity on bottles o 3M HCl (3M Hydrochloric Acid) Molarity = Units are A 3M solution is read as a 3 molar solution There is a distinction between mole and molar Moles represent a Molarity represents a So 0.1M is a concentration of moles / 1 liter of solution, it does not mean.1 moles. 19

20 Example: Definition says Make a 1M solution using KBr 1 mole of KBr Liter or 1000 ml H2O What units do we weigh in? grams How do we convert moles to grams?? Convert 1 mole of KBr to grams: Moles x Molar Mass K = Br = grams / mole Weigh grams of KBr Put it into a 1 Liter volumetric flask Fill to line Shake until dissolved 20

21 Making Solutions: 1. Determine the grams of solute needed to make 1.00 L of a 1.0 M solution of NaCl 2. Determine the grams of solute needed to make 1.00 L of a 0.50 M solution of NaNO3. 3. Determine the grams of solute needed to make ml of a 1.00 M solution of Al(OH)3. 4. Determine the grams of solute needed to make ml of a 0.20 M solution of KI. 21

22 Molarity Problems 1. Determine the number of grams of H 2 SO 4 needed to prepare 1.00 liter of a 2.50M solution of H 2 SO Determine the number of grams of aluminum sulfate needed to prepare 1.00 liter of a 0.025M aluminum sulfate solution. 3. Determine the number of grams of phosphoric acid needed to prepare ml of a 1.00M phosphoric acid solution. 4. Determine the number of grams of calcium hydroxide needed to prepare ml of a 0.100M calcium hydroxide solution moles of nitric acid molecules are dissolved in 1.50 L of water. What is the molarity of this solution. 22

23 Molarity Problems (SHOW ALL WORK) 1. How many grams of CaCl2 would be required to produce a 3.50 M solution with a volume of 2.00 liters? 2. What is the molarity of a.50 Liter solution containing grams of KI? 3. How many moles of LiF would be required to make a 2.50 M solution with a volume of 1.50 Liters? 4. A sample of NaNO3 weighing 8.50 grams is placed in a ml flask. Distilled water is added to the mark on the neck. What is the molarity of this solution? 5. How many grams of NaI would be needed to produce a M solution with a volume of Liters? 6. How many moles of Sr(NO3)2 would be used in the preparation of 10.0 Liters of a 6.00 M solution? 23

24 More Practice 1. What is the equation for Molarity? 2. What is the molarity of a solution if 5.30 g of Na 2 CO 3 is dissolved in ml of water? 3. How many moles of NaCl are contained in ml of a.200m solution? 4. What weight (in grams) of H 2 SO 4 would be needed to make ml of a 2.00M solution? 5. What volume (in ml) of water would be needed if you had 2.45 grams of H 2 SO 4 to make a 18.0 M solution? (see #4 for molar mass of Sulfuric acid) 6. What is the molarity of a solution made by dissolving 20.0 g of H3PO4 in ml of water? 24

25 Dilution 1. What is the equation for dilution? 2. What volume of M KCl is needed to make ml of 0.100M KCl solution? 3. Concentrated H2SO4 is 18.0 M. What volume of 18.0 M solution is needed to make 2.00 L of 1.00 M H 2 SO 4 solution? 4. Concentrated HCl is 12.0 M. If ml of this 12.0 M solution are diluted to ml, what is the molarity of this diluted solution? L of 0.800M KNO 3 are prepared using ml of a more concentrated KNO 3 solution. What is the molarity of this solution? 6. A M solution is to be diluted to a solution. If the original volume is 844 ml, what is the volume after the dilution? 25

26 More Dilution! 1. If I add 25.0 ml of water to ml of a M NaOH solution, what will the molarity of the diluted solution solution be? 2. If I add water to ml of a M NaOH solution until the final volume is ml, what will the molarity of the diluted solution be? 3. How much M HCl solution can be made by diluting ml of 10.0 M HCl? 4. I have ml of a 1.50 M NaCl solution. If I boil the water until the volume of the solution is ml, what will the molarity of the solution be? 5. How much water would I need to add to ml of a 2.40 M KCl solution to make a 1.00 M solution? 26

27 Titration for Acids and Bases Titration is a method used to determine the concentration of an unknown acid (hydronium ion H 3 O + or H + ) or base (hydroxide OH - ). Starting with a solution of unknown concentration of acid or base, small volumes of a solution of known concentration (titrant) are added until an equivalence point or a neutralization point is reached. Typically, the titrant is a strong acid or base. To help determine when the equivalence point occurs, indicators are used. The indicator used will depend on the system being studied since they all change color at slightly different phs. The indicator should have its color change near the equivalence point of the reaction. Some examples: Indicator Color in Acid Color in Base Litmus paper Red Blue Methyl Orange Pink Yellow Phenolphthalein Colorless Magenta When the indicator changes color, the hydronium or hydroxide ions in the unknown solution have been neutralized. The method of expressing concentration of the solution is Normality (N). Normality is expressed as equivalence of solute per liter of solution. Equivalence is related to the number of H 3 O + or OH - that are available for neutralization. H 2 SO 4 has 2 equivalence of H + Al(OH) 3 has 3 equivalence of OH - ** For General Chemistry we will limit the equivalence to 1 so Normality is Molarity ** 27

28 Titration Technique Typically, the unknown solution and the indicator are in the flask and the known solution is put into the buret. There are several steps used to prepare the buret for the titration. 1. Rinse the buret several times with the titrant (approximately 5 ml each time) to be used in the analysis. Use the stopcock to ensure the whole buret has been rinsed, including the tip. Discard all of this titrant into a waste beaker. 2. Drain several milliliters of titrant through the tip using the stopcock to remove any air bubbles that might be present. Again, dispose this titrant into the waste beaker. 3. Fill up the buret, but the level of the titrant must be on the buret scale. Record this initial reading (see top of next page) 4. Repeat steps 1 3 for the unknown solution. 28

29 In order to get accurate data, one must know how to read the level of the solution in the buret. The level of the liquid in the buret is not a straightl line. It is actually a curved line called a meniscus. The meniscus should be viewed at eye level. The correct way to read a meniscus is to observe where its lowest point is and take a reading. One should always estimate the last digit of the value taken. It can be helpful to hold a white card behind the buret to make the meniscus easier to read. First, we need to put a measured amount of the unknown solution into a flask. This value will be given to us. After adding the given amount, another accurate reading should be taken. This is the volume for the unknown solution (VB). The Molarity (MB) will be solved for at the end of the experiment. Next 2 or 3 drops of indicator are added to the flask. The flask is then placed under the buret that contains the titrant or known solution. Slowly, the known solution is added to the liquid in the flask remember we are looking for the equivalence point where we will see a color change based on our indicator. The flask must be swirled at all times while the titrant is being added. **It can also be helpful to place a white piece of paper underneath the flask to help identify when the color change happens. You are only looking for a slight color change for the equivalence point. A bold color change indicates that you went too far with the titration. Lighter is better!!! The color has to stay for 30 seconds. 29

30 You shouldn t add the titrant too fast because it is easy to add too much, but if you add it too slowly, the titration could take a long, long time. So, you can add the titrant steadily until the color starts to hang around for a while but still disappears. At this point, it should be added drop wise until the desired color change occurs. Take an accurate buret reading of the titrant when a slight but constant color change appears. This buret value is MA and VA should have been given since it was the titrant. Using the following equation to solve for the Normality (MB) of the unknown solution: MA x VA = MB x VB Where MA is the Molarity of the acid, VA is the volume of the acid used, MB is the Molarity of the base and VB is the volume of the base used. Solving for MB : (MA X VA) VB Here are a couple of examples to practice using the above equation: Example 1: It takes 15 ml vinegar to neutralize 25 ml of.5m Cd(OH)2. What is the molarity of the vinegar? Example 2: How many ml of.02m KOH will neutralize 15 ml of.4m H2SO4? 30

31 Name Questions on the titration reading 1. What is titration? 2. What is the titrant and what type of compounds are used as titrants usually? 3. What types of materials are used for the equivalence point and why are they used? 4. Normality (N) = 5. Draw a sketch of a titration set up 6. Why should we rinse the buret before using it for a titration? 7. Do you need to record the initial level of titrant? 8. What is a meniscus and how should it be read? 9. How much indicator is added and where is it added? 10. Why do we put white paper under the flask? 11. Why do we swirl the flask while adding titrant? 12. What does a bold color change indicate? 13. Describe the procedure for adding the titrant. 31

32 14. What do the variables in the equation MA x VA = MB x VB represent? MA VA MB VB 15. Rearrange the equation so you can solve for MB MB 32

33 Titration Calculations Acid side = Base side [H + ] = [OH - ] Molarity Acid x Volume Acid = Molarity Base x Volume Base Molarity = moles of acid liters of solution So, Molarity of acid x Volume acid = Molarity of base x Volume base moles of acid x Liters = moles of base x Liters Liters of solution Liters of solution All calculations should be done using a balanced equation 33

34 Name Titration calculations 1. What volume of M HNO 3 will be required to react with ml of M KOH? 2. What volume of M NaOH will be required to neutralize ml of M HClO 4? 3. What is the molarity of HCl if it takes 31.7 ml of the acid to neutralize 15.9 ml of 1.50M LiOH? 4. It takes 28.3 ml of 3.00M HBrO 3 to neutralize 42.5 ml of a RbOH solution. What is the molarity of this base solution? 34

35 Using titration. Solving for the Molarity of an Acid In an Erlenmyer flask: 1. Using a pipetor, add mls of HCl with an unknown molarity. Liquid of known concentration 2. Add ml of dionized water using a graduated cylinder 3. Add 3 drops of phenolphthalein indicator Liquid of unknown concentration In a Buret: 1. Using 5 ml of.05m NaOH rinse the buret 2. Fill to the 0.00 line with 0.05M NaOH 3. With the erlenmeyer flask under the buret, open the stopcock slowly and with constant swirling add NaOH to the acid solution. Slow down the addition of the NaOH as the color change takes longer to disappear. 4. Stop when you see a LIGHT magenta color. The color must stay for at least 30 seconds. If it doesn t, keep adding titrant dropwise until it does. 5. Titrations should always be done at least twice.repeat steps 2 4 At the neutralization point, where the color changes the concentration of Base = the concentration of Acid: [Base] = [Acid] Molarity base x Equivalence base x Volume base = Molarity acid x Equivalence acid X Volume acid Solve for Molarityacid 35

36 Name % Acetic Acid in Vinegar Problem: Using titration, is it possible to determine the % acetic acid (HC2H3O2) in vinegar accurately (+/- 5%)? **Since acetic acid and sodium hydroxide are monoprotic normality = molarity Background: (3 good sentences about titration) Procedure: 1. Fill the buret with.50m NaOH. Record the initial reading on the buret in the table below. 2. Withdraw ml of vinegar (use 5 ml pipette 3 times). Put into a 125 Erlenmeyer flask. Add 20 ml deionized H2O to the flask using a graduated cylinder. 3. Add 3 drops of phenolphthalein to the flask. 4. Put a piece of white paper under the flask. Titrate with NaOH; swirl the flask frequently. Add the NaOH drop by drop near the end point. The solution should be a light pink color at the end point. 5. Discard the solution in the flask down the drain, rinse the flask thoroughly and run a second titration. Observations: Concentration of NaOH (MB) Volume of Acid Used (vinegar) (VA) Volume of Base Used (NaOH) (VB) Trial One Trial Two Average End Value Start Value Total End Value Start Value Total Calculations: 1. Solve the following equation for MA : MA x VA = MB x VB MA = 2. Determine % Acetic Acid % HC2H3O2 = (MA x 60) / 10 OVER 36

37 Conclusions: Calculate % error on your % Acetic Acid value: Accepted Value - Experimental Value % error = x 100 Accepted Value Where accepted value = the value of acetic acid off of the label on the bottle experimental value = the number you determined under calculations. List places where error occurred in this experiment:

38 When Life Gives You Lemonade - Titration Purpose: To practice proper titration technique To determine amount of citric acid (H 3 C 6 H 5 O 7 ) in Crystal Light lemonade Materials: A delicious cup full of Lemonade Phenolphthalein M NaOH dh 2 O buret 250 ml Erlenmeyer flask ml volumetric pipet and pipet pump Procedure: 1. Rinse a buret with dh 2 O then with a small amount of M NaOH. 2. Fill the buret with M NaOH and record the initial volume. 3. Add ml of lemonade and 20.0mL of dh 2 O to a 250 ml flask and a few drops of phenolphthalein indicator. 4. Titrate to a faint pink endpoint then record final volume. 5. Perform two more trials with ml and ml of lemonade respectively. Data and calculations table: (see the back of this lab sheet for calculations!) Trial Volume of Lemonade (ml) Concentration of NaOH (mol/l=m) Initial volume of NaOH (ml) Final volume of NaOH (ml) Volume of NaOH used (ml) Vb Va Mb

39 Citric Acid Lab Calculations: M A x V A = M B x V B Trial 1: M a = Trial 2: M a = Trial 3: M a = 39

40 Titration and Naming Review: Background: The goal of a titration is to use a known concentration of an acid/base to find the unknown concentration of an acid/base. The solution with the known concentration is called the titrant and is put into the buret. The solution with the unknown concentration is put into the erylenmyer flask with an indicator that changes color at the equivalence point. The equivalence point (neutralization point) is when the concentration of base (OH - ) equals the concentration of the acid (H + / H3O + ). The following set-up contains a buret, erlenmeyer flask, and a beaker. Use these pieces of equipment to answer the following questions. 1. What needs to be rinsed with titrant prior to using? 2. Where does the titrant go? 3. Where does the indicator go? 4. Where does the excess titrant go 5. Where does the substance with unknown concentration go? 6. What is the equivalence point of a titration? 7. What are the products of a neutralization reaction? (acid + base ) 8. What color does litmus paper turn with an acid? a base? You must use the following equation to determine the concentration of the unknown solution: MA VA = MB VB Where M= molarity, V = volume, A = acid and B = base. Volume does not need to be in liters. 1. What volume of 0.300M HNO 3 will be required to react with ml of 0.250M KOH? 2. What volume of 0.250M NaOH will be required to neutralize ml of M HClO 4? 3. What is the concentration of HCl, if ml of HCl was neutralized with ml of 0.500M KOH? 40

41 4. Lab titration problem: Starting volume of acid on buret= 0.00mL Ending volume of acid on buret= 17.84mL Molarity of acid= 3.56M Volume of unknown base concentration used= 13.00mL What is the Molarity of the base? Naming acids and bases: Convert Formulas to Names: 5. HBrO 4 6. Mg(OH) 2 7. H 2CO 2 8. H 2CrO 2 9. HBr 10. H 3PO 4 Convert Names to Formulas: 11. Hydrofluoric acid 12. Potassium hydroxide 13. Iodous acid 14. Persulfuric acid 15. Hyponitrous acid 16. Chloric acid 41