Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates

Transcription

1 Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates For Practice 15.1 In each reaction, identify the Brønsted Lowry acid, the Brønsted Lowry base, the conjugate acid, and the conjugate base. a. b.

2 Example 15.2 Using K w in Calculations For Practice 15.2 Calculate [H 3 O + ] at 25 C for each solution and determine if the solution is acidic, basic, or neutral. a. [OH ] = M b. [OH ] = M c. [OH ] = M

3 Example 15.3 Calculating ph from [H 3 O + ] or [OH ] For Practice 15.3 Calculate the ph of each solution and indicate whether the solution is acidic or basic. a. [H 3 O + ] = M b. [OH ] = M

4 Example 15.4 Calculating [H 3 O + ] from ph For Practice 15.4 Calculate the [H 3 O + ] for a solution with a ph of 8.37.

5 Example 15.5 Finding the [H 3 O + ] of a Weak Acid Solution For Practice 15.5 Find the H 3 O + concentration of a M hydrofluoric acid solution.

6 Example 15.6 Finding the ph of a Weak Acid Solution For Practice 15.6 Find the ph of a M acetic acid solution.

7 Example 15.7 Finding the ph of a Weak Acid Solution in Cases Where the x is small Approximation Does Not Work For Practice 15.7 Find the ph of a M HNO 2 solution.

8 Example 15.8 Finding the Equilibrium Constant from ph For Practice 15.8 A M weak acid solution has a ph of Find K a for the acid.

9 Example 15.9 Finding the Percent Ionization of a Weak Acid For Practice 15.9 Find the percent ionization of a M HC 2 H 3 O 2 solution at 25 C.

10 Example Mixtures of Weak Acids For Practice Find the ClO concentration of the above mixture of HF and HClO.

11 Example Finding the [OH ] and ph of a Strong Base Solution For Practice Find the [OH ] and ph of a M Ba (OH) 2 solution.

12 Example Finding the [OH ] and ph of a Weak Base Solution For Practice Find the [OH ] and ph of a 0.33 M methylamine solution.

13 Example Determining Whether an Anion Is Basic or ph-neutral For Practice Classify each anion as a weak base or ph-neutral: a. CHO 2 b. ClO 4

14 Example Determining the ph of a Solution Containing an Anion Acting as a Base For Practice Find the ph of a M NaC 2 H 3 O 2 solution.

15 Example Determining Whether a Cation Is Acidic or ph-neutral For Practice Classify each cation as a weak acid or ph-neutral. a. Li + b. CH 3 NH 3 + c. Fe 3+

16 Example Determining the Overall Acidity or Basicity of Salt Solutions For Practice Determine if the solution formed by each salt is acidic, basic, or neutral. a. NaHCO 3 b. CH 3 CH 2 NH 3 Cl c. KNO 3 d. Fe(NO 3 ) 3

17 Example Finding the ph of a Polyprotic Acid Solution For Practice Find the ph of a M H 2 CO 3 solution.

18 Example Dilute H 2 SO 4 Solutions For Practice Find the ph and [SO 4 2 ] of a M sulfuric acid solution.

19 Example Finding the Concentration of the Anions for a Weak Diprotic Acid Solution For Practice Find the [CO 3 2 ] of the M carbonic acid (H 2 CO 3 ) solution in For Practice

20 Example 16.1 Calculating the ph of a Buffer Solution For Practice 16.1 Calculate the ph of a buffer solution that is M in HC 2 H 3 O 2 and M in NaC 2 H 3 O 2. For More Practice 16.1 Calculate the ph of the buffer that results from mixing 60.0 ml of M HCHO 2 and 15.0 ml of M NaCHO 2.

21 Example 16.2 Calculating the ph of a Buffer Solution as an Equilibrium Problem and with the Henderson Hasselbalch Equation For Practice 16.2 Calculate the ph of a buffer solution that is M in HCN and M in KCN. For HCN, K a = (pk a = 9.31). Use both the equilibrium approach and the Henderson Hasselbalch approach.

22 Example 16.3 Calculating the ph Change in a Buffer Solution after the Addition of a Small Amount of Strong Acid or Base For Practice 16.3 Calculate the ph of the solution in Example 16.3 upon addition of mol of NaOH to the original buffer. For More Practice 16.3 Calculate the ph of the solution in Example 16.3 upon addition of 10.0 ml of 1.00 M HCl to the original buffer in Example 16.3.

23 Example 16.4 Using the Henderson Hasselbalch Equation to Calculate the ph of a Buffer Solution Composed of a Weak Base and Its Conjugate Acid For Practice 16.4 Calculate the ph of 1.0 L of the solution in Example 16.4 upon addition of mol of solid NaOH to the original buffer solution. For More Practice 16.4 Calculate the ph of 1.0 L of the solution in Example 16.4 upon addition of 30.0 ml of 1.0 M HCl to the original buffer solution.

24 Example 16.5 Preparing a Buffer For Practice 16.5 Which acid in Example 16.5 would you choose to create a buffer with ph = 7.35? If you have ml of a 0.10 M solution of the acid, what mass of the corresponding sodium salt of the conjugate base do you need to make the buffer?

25 Example 16.6 Strong Acid Strong Base Titration ph Curve For Practice 16.6 Calculate the ph in the titration in Example 16.6 after the addition of 60.0 ml of M HNO 3.

26 Example 16.7 Weak Acid Strong Base Titration ph Curve For Practice 16.7 Determine the ph at the equivalence point for the titration of HNO 2 and KOH in Example 16.7.

27 Example 16.8 Calculating Molar Solubility from K sp For Practice 16.8 Calculate the molar solubility of Fe(OH) 2 in pure water.

28 Example 16.9 Calculating K sp from Molar Solubility For Practice 16.9 The molar solubility of AgBr in pure water is M. Calculate K sp.

29 Example Calculating Molar Solubility in the Presence of a Common Ion For Practice Calculate the molar solubility of CaF 2 in a solution containing M Ca(NO 3 ) 2.

30 Example The Effect of ph on Solubility For Practice Which compound, FeCO 3 or PbBr 2, is more soluble in acid than in base? Why?

31 Example Predicting Precipitation Reactions by Comparing Q and K sp For Practice If the original solutions in Example are concentrated through evaporation and mixed again to form a solution that is M in Pb(NO 3 ) 2 and M in NaBr, will a precipitate form in this newly mixed solution?

32 Example Finding the Minimum Required Reagent Concentration for Selective Precipitation For Practice If the concentration of Mg 2+ in the previous solution was M, what minimum [OH ] triggers precipitation of the Mg 2+ ion?

33 Example Finding the Concentrations of Ions Left in Solution after Selective Precipitation For Practice A solution is M in Pb 2+ and M in Ag +. (a) If selective precipitation is to be achieved using NaCl, what minimum concentration of NaCl do you need to begin to precipitate the ion that precipitates first? (b) What is the concentration of each ion left in solution at the point where the second ion begins to precipitate?

34 Example Complex Ion Equilibria For Practice You mix a ml sample of a solution that is M in NiCl 2 with a ml sample of a solution that is M in NH 3. After the solution reaches equilibrium, what concentration of Ni 2+ (aq) remains?