Write the balanced NET IONIC equation for the reaction that occurs when hydrochl

Question

Write the balanced NET IONIC equation for the reaction that occurs when hydrochloric acid and potassium fluoride are combined.

Use H3O+ instead of H+


This reaction is classified as.
A. Strong Acid + Strong Base
B. Weak Acid + Strong Base
C. Strong Acid + Weak Base
D. Weak Acid + Weak Base

The extent of this reaction is:.
A. ... Below 50%
B. ... 50%
C. ... Above 50%
D. ... 100%

B---Determine the pH change when 0.094 mol NaOH is added to 1.00 L of a buffer solution that is 0.370 M in HCN and 0.306 M in CN-.

C----A buffer solution contains 0.500 M CH3NH3Br and 0.376 M CH3NH2 (methylamine). Determine the pH change when 0.081 mol NaOH is added to 1.00 L of the buffer.

Explanation / Answer

HCl(aq) + KF(aq) ----> HF(aq) + KCl(aq)

net ionic equation

H^+(aq) + F^-(aq) ----> HF(aq)

c . strong acid + weak base.

100%

B) pka of HCN = 9.31

   pH = pka + log(salt/acid)

    = 9.31 + log(0.306/0.37)

   = 9.23

after adding 0.094 mol NaOH

     = 9.31 + log((0.306+0.094)/(0.37-0.094))

   = 9.47

change in pH = 9.47-9.23 = 0.24

c) pH = 14-pkb+log(salt/base)

pkb of CH3NH2 = 3.38

       = 14 - (3.38+log(0.5/0.376))

      = 10.5

after addition of 0.081 mol NaOH

   = 14 - (3.38+log((0.5-0.081)/(0.376+0.081)))

      = 10.66

CHANGE in pH = 10.66-10.5 = 0.16

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