Question

Calculate the [H+] and pH of a 0.0035 M nitrous acid solution. The $K_a$ of nitrous acid is $7.10 \times 10^{-4}$. Use the method of successive approximations in your calculations. 0.00159 [H+] = Incorrect Answer 2.804 pH = Correct Answer M

          Calculate the [H+] and pH of a 0.0035 M nitrous acid solution. The $K_a$ of nitrous acid is $7.10 \times 10^{-4}$. Use the method of successive approximations in your calculations.
0.00159
[H+] = 
Incorrect Answer
2.804
pH = 
Correct Answer
M

Calculate the [H+] and pH of a 0.0035 M nitrous acid solution. The Ka of nitrous acid is 7.10 × 10^-4. Use the method of successive approximations in your calculations.
0.00159
[H+] =
Incorrect Answer
2.804
pH =
Correct Answer
M

Added by Andrea K.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sima Sarker

11/04/2023

Step 1

10 \times 10^{-4}$ and $[HNO_2] = 0.0035 M$. Let x be the concentration of $[H^+]$ and $[NO_2^-]$. Then, $[HNO_2] = 0.0035 - x$. $7.10 \times 10^{-4} = \frac{x^2}{0.0035 - x}$ Show more…

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Calculate the [H+] and pH of a 0.0035 M nitrous acid solution. The $K_a$ of nitrous acid is $7.10 \times 10^{-4}$. Use the method of successive approximations in your calculations. 0.00159 [H+] = Incorrect Answer 2.804 pH = Correct Answer M