Problem: Calculate the pH of a solution made by mixing 49.5 mL of 0.335 M NaA (Ka for HA = 1.0 × 10–9) with 30.6 mL of 0.120 M HCl.A) 9.00B) 9.65C) 8.45D) 8.75E) 9.55

FREE Expert Solution

For this problem, we have to calculate the pH when 49.5 mL of 0.335 M NaA is mixed with 30.6 mL of 0.120 M HCl.

  • NaA is a basic salt that reacts with HCl (strong acid) as:

NaA (aq) + HCl (aq) →   HA (aq) + NaCl (aq) 

  • In this case, we have to calculate the moles of Ainitially and moles of HCl added to the mixture

Step 1. Find the moles of Aand Hfrom HCl

Step 2. Construct an ICF chart

Step 3. Calculate the pH


(1) Moles of Awill be calculated as:

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Problem Details

Calculate the pH of a solution made by mixing 49.5 mL of 0.335 M NaA (Ka for HA = 1.0 × 10–9) with 30.6 mL of 0.120 M HCl.

A) 9.00

B) 9.65

C) 8.45

D) 8.75

E) 9.55

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Base Strong Acid Titrations concept. You can view video lessons to learn Weak Base Strong Acid Titrations. Or if you need more Weak Base Strong Acid Titrations practice, you can also practice Weak Base Strong Acid Titrations practice problems.