30 ml of 0.1N HCI is added from burette into 20 ml of 0.11 N NaHCO3solutions in flask. Calculate pH of the titration mixture.
Question
Solution 1
To calculate the pH of the titration mixture, we first need to determine the moles of HCl and NaHCO3.
-
Calculate the moles of HCl and NaHCO3:
Moles of HCl = Normality x Volume(L) = 0.1N x 30/1000 L = 0.003 moles Moles of NaHCO3 = Normality x Volume(L) = 0.11N x 20/1000 L = 0.0022 moles
2 Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI
Similar Questions
30 ml of 0.1N HCI is added from burette into 20 ml of 0.11 N NaHCO3solutions in flask. Calculate pH of the titration mixture.
2 H2O2(l) 2 H2O(g) + O2(g) Decompose 0.11 g of H2O2 in a flask with a volume of 2500.0 mL. What is the pressure of O2 at 25 oC? Of H2O?
A 20.00 mL sample of 0.150 M NH3 is being titrated with 0.200 M HCl. What is the pH after 10.00 mL of HCl has been added? Kb of NH3 = 1.8 × 10−5
What is the pH of 0.11 M solution of Ca(OH)2 [log 11 = 1.041]Select an answerA0.65 B0.95C2D0.3010
When 2.35g Mg(OH)2 is added to 250.0 mL of water, the temperature of the waterraises from 20.5oC to 36.0oC. Calculate the molar enthalpy of solution.
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.