Determine whether each of the following is true or false: (a) All strong bases are salts of the hydroxide ion. (b) The addition of a strong base to water produces a solution of pH > 7.0. (c) Because Mg(OH)2 is not very soluble, it can- not be a strong base. 16.43 Calculate the pH of each of the following strong acid solu- tions: (a) 8.5 x 10-3M HBr, (b) 1.52 g of HNO3 in 575 mL of solution, (c) 5.00 mL of .250 M HCIO4 diluted to 50.0 mL, (d) a solution formed by mixing 10.0 mL of 0.100 M HBr with 20.0 mL of 0.200 M HCI. 16.44 Calculate the pH of each of the following strong acid solu- tions: (a) 0.0167 M HNO3, (b) 0.225 g of HCIO3 in 2.00 L of solution, (c) 15.00 mL of 1.00 M HCl diluted to 0.500 L, (d) a mixture formed by adding 50.0 mL of 0.020 M HCl to 125 mL of 0.010 M HI. 16.45 Calculate [OH ] and pH for (a) 1.5 × 10³M Sr(OH)2, (b) 2.250 g of LiOH in 250.0 mL of solution, (c) 1.00 mL of 0.175 M NAOH diluted to 2.00 L, (d) a solution formed by adding 5.00 mL of 0.105 M KOH to 15.0 mL of 9.5 × 10-2 M Ca(OH)2. 16.46 Calculate [OH¯] and pH for each of the following strong base solutions: (a) 0.182 M KOH, (b) 3.165 g of KOH in 500.0 mL of solution, (c) 10.0 mL of 0.0105 M Ca(OH)2 diluted to 500.0 mL, (d) a solution formed by mixing 20.0 mL of 0.015 M Ba(OH)2 with 40.0 mL of 8.2 × 103 M NaOH. 16.47 Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50. 16.48 Calculate the concentration of an aqueous solution of Ca(OH)2 that has a pH of 10.05. Weak Acids (Section 16.6) 16.49 Write the chemical equation and the Ka expression for the ionization of each of the following acids in aqueous solu- tion. First show the reaction with H"(aq) as a product and then with the hydronium ion: (a) HBrO2, (b) C,H5COOH.
Determine whether each of the following is true or false: (a) All strong bases are salts of the hydroxide ion. (b) The addition of a strong base to water produces a solution of pH > 7.0. (c) Because Mg(OH)2 is not very soluble, it can- not be a strong base. 16.43 Calculate the pH of each of the following strong acid solu- tions: (a) 8.5 x 10-3M HBr, (b) 1.52 g of HNO3 in 575 mL of solution, (c) 5.00 mL of .250 M HCIO4 diluted to 50.0 mL, (d) a solution formed by mixing 10.0 mL of 0.100 M HBr with 20.0 mL of 0.200 M HCI. 16.44 Calculate the pH of each of the following strong acid solu- tions: (a) 0.0167 M HNO3, (b) 0.225 g of HCIO3 in 2.00 L of solution, (c) 15.00 mL of 1.00 M HCl diluted to 0.500 L, (d) a mixture formed by adding 50.0 mL of 0.020 M HCl to 125 mL of 0.010 M HI. 16.45 Calculate [OH ] and pH for (a) 1.5 × 10³M Sr(OH)2, (b) 2.250 g of LiOH in 250.0 mL of solution, (c) 1.00 mL of 0.175 M NAOH diluted to 2.00 L, (d) a solution formed by adding 5.00 mL of 0.105 M KOH to 15.0 mL of 9.5 × 10-2 M Ca(OH)2. 16.46 Calculate [OH¯] and pH for each of the following strong base solutions: (a) 0.182 M KOH, (b) 3.165 g of KOH in 500.0 mL of solution, (c) 10.0 mL of 0.0105 M Ca(OH)2 diluted to 500.0 mL, (d) a solution formed by mixing 20.0 mL of 0.015 M Ba(OH)2 with 40.0 mL of 8.2 × 103 M NaOH. 16.47 Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50. 16.48 Calculate the concentration of an aqueous solution of Ca(OH)2 that has a pH of 10.05. Weak Acids (Section 16.6) 16.49 Write the chemical equation and the Ka expression for the ionization of each of the following acids in aqueous solu- tion. First show the reaction with H"(aq) as a product and then with the hydronium ion: (a) HBrO2, (b) C,H5COOH.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 107AP
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Question
16.44 (c)
![Determine whether each of the following is true or false:
(a) All strong bases are salts of the hydroxide ion. (b) The
addition of a strong base to water produces a solution of
pH > 7.0. (c) Because Mg(OH)2 is not very soluble, it can-
not be a strong base.
16.43 Calculate the pH of each of the following strong acid solu-
tions: (a) 8.5 x 10-3M HBr, (b) 1.52 g of HNO3 in 575 mL of
solution, (c) 5.00 mL of .250 M HCIO4 diluted to 50.0 mL,
(d) a solution formed by mixing 10.0 mL of 0.100 M HBr
with 20.0 mL of 0.200 M HCI.
16.44 Calculate the pH of each of the following strong acid solu-
tions: (a) 0.0167 M HNO3, (b) 0.225 g of HCIO3 in 2.00 L
of solution, (c) 15.00 mL of 1.00 M HCl diluted to 0.500 L,
(d) a mixture formed by adding 50.0 mL of 0.020 M HCl to
125 mL of 0.010 M HI.
16.45 Calculate [OH ] and pH for (a) 1.5 × 10³M Sr(OH)2,
(b) 2.250 g of LiOH in 250.0 mL of solution, (c) 1.00
mL of 0.175 M NAOH diluted to 2.00 L, (d) a solution
formed by adding 5.00 mL of 0.105 M KOH to 15.0 mL of
9.5 × 10-2 M Ca(OH)2.
16.46 Calculate [OH¯] and pH for each of the following strong
base solutions: (a) 0.182 M KOH, (b) 3.165 g of KOH in 500.0
mL of solution, (c) 10.0 mL of 0.0105 M Ca(OH)2 diluted to
500.0 mL, (d) a solution formed by mixing 20.0 mL of 0.015
M Ba(OH)2 with 40.0 mL of 8.2 × 103 M NaOH.
16.47 Calculate the concentration of an aqueous solution of
NaOH that has a pH of 11.50.
16.48 Calculate the concentration of an aqueous solution of
Ca(OH)2 that has a pH of 10.05.
Weak Acids (Section 16.6)
16.49 Write the chemical equation and the Ka expression for the
ionization of each of the following acids in aqueous solu-
tion. First show the reaction with H"(aq) as a product and
then with the hydronium ion: (a) HBrO2, (b) C,H5COOH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb2f71cc3-406d-4549-a751-96d454552a8c%2Fcf489be8-6e39-42b8-b79e-0f8d4f00b3d6%2F60d0zhu.jpeg&w=3840&q=75)
Transcribed Image Text:Determine whether each of the following is true or false:
(a) All strong bases are salts of the hydroxide ion. (b) The
addition of a strong base to water produces a solution of
pH > 7.0. (c) Because Mg(OH)2 is not very soluble, it can-
not be a strong base.
16.43 Calculate the pH of each of the following strong acid solu-
tions: (a) 8.5 x 10-3M HBr, (b) 1.52 g of HNO3 in 575 mL of
solution, (c) 5.00 mL of .250 M HCIO4 diluted to 50.0 mL,
(d) a solution formed by mixing 10.0 mL of 0.100 M HBr
with 20.0 mL of 0.200 M HCI.
16.44 Calculate the pH of each of the following strong acid solu-
tions: (a) 0.0167 M HNO3, (b) 0.225 g of HCIO3 in 2.00 L
of solution, (c) 15.00 mL of 1.00 M HCl diluted to 0.500 L,
(d) a mixture formed by adding 50.0 mL of 0.020 M HCl to
125 mL of 0.010 M HI.
16.45 Calculate [OH ] and pH for (a) 1.5 × 10³M Sr(OH)2,
(b) 2.250 g of LiOH in 250.0 mL of solution, (c) 1.00
mL of 0.175 M NAOH diluted to 2.00 L, (d) a solution
formed by adding 5.00 mL of 0.105 M KOH to 15.0 mL of
9.5 × 10-2 M Ca(OH)2.
16.46 Calculate [OH¯] and pH for each of the following strong
base solutions: (a) 0.182 M KOH, (b) 3.165 g of KOH in 500.0
mL of solution, (c) 10.0 mL of 0.0105 M Ca(OH)2 diluted to
500.0 mL, (d) a solution formed by mixing 20.0 mL of 0.015
M Ba(OH)2 with 40.0 mL of 8.2 × 103 M NaOH.
16.47 Calculate the concentration of an aqueous solution of
NaOH that has a pH of 11.50.
16.48 Calculate the concentration of an aqueous solution of
Ca(OH)2 that has a pH of 10.05.
Weak Acids (Section 16.6)
16.49 Write the chemical equation and the Ka expression for the
ionization of each of the following acids in aqueous solu-
tion. First show the reaction with H"(aq) as a product and
then with the hydronium ion: (a) HBrO2, (b) C,H5COOH.
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