Question

Determine the pH of each of the following solutions.

Part A 0.11 molL−1 NH4Cl Express your answer to two decimal places. Part B 0.20 molL−1 CH3COONa Part C 0.19 molL−1 NaCl

Answer 1

Sol. A

NH4Cl is a salt of strong acid HCl and weak base NH4OH so the salt solution will be acidic.

Also $Cl^-}$ will not effect the ph of the solution.

Pavs A ol mol U N a Dissosdiavion Pam] Nu,u Nu C Tniwal a Eiun X foxNuN ka ka kb kw ka Ol1-X 5.6 x 1o 1o asumiy 5.6 x lo10 X O.185 XI6 C0 .8510- PM--103 M0 X10 5.105 PM 5.105

Sol. B

CH3COONa is a salt of strong base NaOH and weak acid CH3COOH. So the salt solution will be basic in nature.

Also $Na{^+}$ will not effect the ph of the solution.

Pau B O.20 mol L Cu CooNa (Disosd ali on Си, Соо Na* CyCoo CJongaon Rm Ou Сизсоои + So Imive! O.20 X X 20-X a Eium kb=[o] Ce Coou 5. 6x10 2 ko:kdo ku - 19 6. 20 - 5.6 x1010 auumi X 2S 20 X Cой] Pov lo3 (105 x103) =4.978 Pu-t Pou19 14-4.91 8 PM

Sol. C

NaCl is the salt of strong base NaOH and strong acid HCl so both will not be neutralising each other and hence the solution will be neither acidic and nor basic.

So the ph will be $7$.