What is the pH of a solution obtained by mixing 155 mL of 0.5 M CH_3NH_2 and 173

Question

What is the pH of a solution obtained by mixing 155 mL of 0.5 M CH_3NH_2 and 173 mL of 1.0 M CH_3NH_3^+CI^-? (K_b for CH_3NH_2 is: 5.2 times 10^-4) Input your answer to 2 decimal places. For example, if the answer is pH = 12, you would input 12.00 QUESTION 8 Following this discussion, we can qualitatively predict the pH of a salt solution: Salt of strong bases and strong acids: neutral a. Eg. NaCI i. NaOH (strong base) and HCI (strong acid) Salt of strong bases and weak acids: basic a. Eg. NaOCH_3 i. NaOH (strong base) and HOCH_3 (weak acid) Salt of weak bases and strong acids: acidic NH_4CI a. Eg. NH_4CI i. NH_4OH (weak base) and HCI (strong acid) Predict the pH of an aqueous solution of NH_4NO_3: 1. PH is less than 7 2. pH =7 3. pH is greater than 7

Explanation / Answer

7 )

pKb = 3.28

pOH = pKb + log (salt / base)

pOH = 3.28 + log (173 x 1.0 / 155 x 0.5)

pOH = 3.63

pH + pOH = 14

pH = 10.37 --------------------> answer

Q 8)

NH4NO3 is the weak base and strong acid so pH <7

1) pH is less than 7 --------------------> answer

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