QuestionJuly 18, 2025

1. Calculate the pH values for the following solutions a) the acid solution with [H^+]=0.002M b) 0.01M HCl aqueous solution c) 0.01 M NaOH aqueous solution d) an aqueous solution with pOH=10.3

1. Calculate the pH values for the following solutions a) the acid solution with [H^+]=0.002M b) 0.01M HCl aqueous solution c) 0.01 M NaOH aqueous solution d) an aqueous solution with pOH=10.3
1. Calculate the pH values for the following solutions a) the acid solution with [H^+]=0.002M b) 0.01M HCl aqueous solution c) 0.01 M NaOH aqueous solution d) an aqueous solution with pOH=10.3

Solution
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Answer

a) 2.7 ### b) 2 ### c) 12 ### d) 3.7 Explanation 1. Calculate pH for [H^{+}]=0.002M Use the formula **pH = -\log[H^+]**. For [H^+] = 0.002M, pH = -\log(0.002) \approx 2.7. 2. Calculate pH for 0.01M HCl HCl is a strong acid, so [H^+] = 0.01M. Use **pH = -\log[H^+]**. pH = -\log(0.01) = 2. 3. Calculate pH for 0.01M NaOH NaOH is a strong base, so [OH^-] = 0.01M. First, calculate pOH = -\log[OH^-] = -\log(0.01) = 2. Then use **pH + pOH = 14** to find pH = 14 - 2 = 12. 4. Calculate pH from pOH=10.3 Use **pH + pOH = 14**. Given pOH = 10.3, pH = 14 - 10.3 = 3.7.

Explanation

1. Calculate pH for $[H^{+}]=0.002M$<br /> Use the formula **$pH = -\log[H^+]$**. For $[H^+] = 0.002M$, $pH = -\log(0.002) \approx 2.7$.<br /><br />2. Calculate pH for 0.01M HCl<br /> HCl is a strong acid, so $[H^+] = 0.01M$. Use **$pH = -\log[H^+]$**. $pH = -\log(0.01) = 2$.<br /><br />3. Calculate pH for 0.01M NaOH<br /> NaOH is a strong base, so $[OH^-] = 0.01M$. First, calculate $pOH = -\log[OH^-] = -\log(0.01) = 2$. Then use **$pH + pOH = 14$** to find $pH = 14 - 2 = 12$.<br /><br />4. Calculate pH from $pOH=10.3$<br /> Use **$pH + pOH = 14$**. Given $pOH = 10.3$, $pH = 14 - 10.3 = 3.7$.
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