Multiple Choice
What is the pH and [OH-] concentration of a solution if the [H3O+] is 4.0 x 10^-9 M?
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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What is the pH of the solution when 150 ml of 3M HCl is mixed with 300 ml of 1.5M NaCN?
A
pH = 11
B
pH = 7
C
pH = 9
D
pH = 1
Verified step by step guidance1
Calculate the moles of HCl using the formula: \( \text{moles of HCl} = \text{volume (L)} \times \text{molarity (M)} \). Convert 150 mL to liters and multiply by 3 M.
Calculate the moles of NaCN using the formula: \( \text{moles of NaCN} = \text{volume (L)} \times \text{molarity (M)} \). Convert 300 mL to liters and multiply by 1.5 M.
Determine the limiting reactant by comparing the moles of HCl and NaCN. The reaction between HCl and NaCN will produce HCN and NaCl.
Calculate the concentration of HCN formed in the solution. Use the total volume of the solution (150 mL + 300 mL converted to liters) to find the concentration of HCN.
Use the concentration of HCN to find the pH. HCN is a weak acid, so use the expression for the ionization of HCN and the acid dissociation constant \( K_a \) to find the concentration of \( H^+ \) ions, and then calculate the pH using \( \text{pH} = -\log[H^+] \).
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