Answer to Question #349492 in General Chemistry for hailey

Question

An aqueous solution of HCl is added to an aqueous solution of Ca(OH) 2 and a reaction occurs. 8.9x10 -

6 mol of (OH – ) ions are measured in the 750mL solution. Remember, Molarity = mol/L. Calculate the

concentration of the H + ions. Is the solution more acidic or basic?

Answer 1

C_M (OH^-) = n / V = 8,9*10^-6 / 0,75 = 1,14*10^-5

pOH = -log (OH^-)

pOH = -log (1,14*10^-5) = 4,94

pH + pOH = 14

pH = 14 - pOH = 14 - 4,94 = 9,06

pH = -log (H⁺)

9,06 = -log (H⁺)

H⁺ = 1,148*10^-10 mol/l

Solution is basic

Answer:

[H⁺]=1,148*10^-10

solution is a basic