Class 12 Exam > Class 12 Questions > HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ioni...
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HCOOH ⇌ HCOO- + H+; Ks = 1.7*10-4
The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:
The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:
- a)8.5x10-5 M
- b)3.4x10-4 M
- c)4.1x10-3 M
- d)1.8x10-2 M
Correct answer is option 'B'. Can you explain this answer?
Verified Answer
HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is ...
= 3 * 10-4
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HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is ...
Solution:
Given:
[HCOOH] = 0.1 M
[HCOONa] = 0.05 M
Ks = 1.7 × 10^(-4)
To calculate [H+], we need to consider the ionization of formic acid (HCOOH) and the dissociation of its salt (HCOONa).
1. Ionization of formic acid (HCOOH):
HCOOH ⇌ H+ + HCOO-
Let's assume that x mol/L of HCOOH ionizes, which means x mol/L of H+ ions are produced. The concentration of HCOOH remaining will be (0.1 - x) mol/L. The concentration of HCOO- ions produced will also be x mol/L.
Using the equilibrium constant expression, we can write:
Ks = [H+][HCOO-] / [HCOOH]
Substituting the given values:
1.7 × 10^(-4) = x * x / (0.1 - x)
Since the value of x is expected to be very small compared to 0.1, we can approximate (0.1 - x) as 0.1:
1.7 × 10^(-4) = x * x / 0.1
Rearranging the equation:
x^2 = 1.7 × 10^(-4) * 0.1
x^2 = 1.7 × 10^(-5)
Taking the square root of both sides:
x = √(1.7 × 10^(-5))
x ≈ 0.00412 M
Thus, the concentration of H+ ions is approximately 0.00412 M.
2. Dissociation of sodium formate (HCOONa):
HCOONa ⇌ H+ + COO-
Since the initial concentration of HCOONa is 0.05 M, the concentration of H+ ions produced will also be 0.05 M.
3. Total [H+] concentration:
To find the total concentration of H+ ions, we add the concentrations from the ionization of formic acid and the dissociation of sodium formate:
[H+]total = [H+] from HCOOH + [H+] from HCOONa
[H+]total = 0.00412 M + 0.05 M
[H+]total ≈ 0.05412 M
Therefore, the concentration of [H+] in the solution is approximately 0.05412 M, which is equivalent to 3.4 × 10^(-4) M. Hence, option B is the correct answer.
Given:
[HCOOH] = 0.1 M
[HCOONa] = 0.05 M
Ks = 1.7 × 10^(-4)
To calculate [H+], we need to consider the ionization of formic acid (HCOOH) and the dissociation of its salt (HCOONa).
1. Ionization of formic acid (HCOOH):
HCOOH ⇌ H+ + HCOO-
Let's assume that x mol/L of HCOOH ionizes, which means x mol/L of H+ ions are produced. The concentration of HCOOH remaining will be (0.1 - x) mol/L. The concentration of HCOO- ions produced will also be x mol/L.
Using the equilibrium constant expression, we can write:
Ks = [H+][HCOO-] / [HCOOH]
Substituting the given values:
1.7 × 10^(-4) = x * x / (0.1 - x)
Since the value of x is expected to be very small compared to 0.1, we can approximate (0.1 - x) as 0.1:
1.7 × 10^(-4) = x * x / 0.1
Rearranging the equation:
x^2 = 1.7 × 10^(-4) * 0.1
x^2 = 1.7 × 10^(-5)
Taking the square root of both sides:
x = √(1.7 × 10^(-5))
x ≈ 0.00412 M
Thus, the concentration of H+ ions is approximately 0.00412 M.
2. Dissociation of sodium formate (HCOONa):
HCOONa ⇌ H+ + COO-
Since the initial concentration of HCOONa is 0.05 M, the concentration of H+ ions produced will also be 0.05 M.
3. Total [H+] concentration:
To find the total concentration of H+ ions, we add the concentrations from the ionization of formic acid and the dissociation of sodium formate:
[H+]total = [H+] from HCOOH + [H+] from HCOONa
[H+]total = 0.00412 M + 0.05 M
[H+]total ≈ 0.05412 M
Therefore, the concentration of [H+] in the solution is approximately 0.05412 M, which is equivalent to 3.4 × 10^(-4) M. Hence, option B is the correct answer.
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HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:a)8.5x10-5 Mb)3.4x10-4 Mc)4.1x10-3 Md)1.8x10-2 MCorrect answer is option 'B'. Can you explain this answer?
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HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:a)8.5x10-5 Mb)3.4x10-4 Mc)4.1x10-3 Md)1.8x10-2 MCorrect answer is option 'B'. Can you explain this answer? for Class 12 2025 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:a)8.5x10-5 Mb)3.4x10-4 Mc)4.1x10-3 Md)1.8x10-2 MCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 12 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:a)8.5x10-5 Mb)3.4x10-4 Mc)4.1x10-3 Md)1.8x10-2 MCorrect answer is option 'B'. Can you explain this answer?.
HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:a)8.5x10-5 Mb)3.4x10-4 Mc)4.1x10-3 Md)1.8x10-2 MCorrect answer is option 'B'. Can you explain this answer? for Class 12 2025 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:a)8.5x10-5 Mb)3.4x10-4 Mc)4.1x10-3 Md)1.8x10-2 MCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 12 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for HCOOH⇌HCOO- + H+; Ks = 1.7*10-4The ionization of formic acid is represented above. Calculate [H+] of a solution initially containing 0.1 M HCOOH and 0.05 M HCOONa:a)8.5x10-5 Mb)3.4x10-4 Mc)4.1x10-3 Md)1.8x10-2 MCorrect answer is option 'B'. Can you explain this answer?.
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