Question

3. Solution A has a hydronium ion concentration of 3.8 x 10® M. Solution B has a hydronium ion concentration of 2.5 x 10M. a. Which solution has the higher hydronium ion concentration? b. Which solution has the higher pH? C. Calculate the pH of the more acidic solution. Show all work. 4. Consider hydrolysis reactions and then predict whether the pH of an aqueous solution of each of the following compounds is greater than 7(>7), less than 7<7), or about 7=7). If a prediction is not possible, write "more info". (See Examples 1 and 2 above for guidance.) a. KNO2 b. CuBr2 c. LINO3

Answer 1

3) a)

Solution B has higher hydronium ion concentration.

b) pH = -log([H+])

solution A. pH = -log(3.8×10^-8) => 7.42

Solution B , pH =-log(2.5×10^-4) => 3.60

solution A has higher pH .

c) As solution B has less pH means it is more acidic.

Solution B , pH = -log([H+])

pH=-log(2.5×10^-4) => 3.60

4) a. As it is basic salt so pH >7

b. It is acidic salt , pH < 7

c. It is neutral salt , pH = 7