Question

pH of Barium hydroxide solution if 10 ml of this neutralises 20 ml of 0.01 M HCl solution 3. A solution of Na2CO3 is prepared by dissolving 0.53 g in 100 ml of the solution. To this 200 ml of 0.001 M NaOH is added. What is the pH of resulting mixture? 4. 100 ml of solution of pH = 2 and 400 ml of solution of pH = 9 are mixed at 25oC. The resulting solution is diluted to one litre. Calculate the pH of solution. 5. What is the pH of solution having [H+] = 2.512 × 10–6 M? 6. What is the pH of a solution containing 0.63 g of HNO3 in 100 ml of solution? 7. Calculate the pH of an aqueous solution having 2g of NaOH per 500 ml of it. 8. 150 ml of 0.5 N HCl and 100 ml of 0.2 N HCl are mixed. Find the pH of the resulting solution? 9. Equal volume of 0.5 N NaOH and 0.3 N KOH are mixed in an experiment. Find the POH & pH of the resulting solution. 10. 50 ml of 0.2 M HCl is added to 30 ml of 0.1 M KOH solution. Find the pH of the solution. 11. 40 ml of 0.2 N HNO3 when reacted with 60 ml of 0.3 M NaOH gave a mixed solution. What is the pH of the solution? 12. Calculate the pH of a 10–5 M HCl solution if 1 ml of it is diluted to 1000 ml. (Kw = 1 × 10-14) 13. Ionic product of water at 310 K is 2.7 × 10-14. What is the pH of neutral water at this temperature?

Answer 1

Answer:

For HCl, Molarity = Normality (since n-factor is 1)

Number of moles of H

+

=M×V=0.1×10×10

−3

=10

−3

Total volume =10+990ml=1 litre

[H

+

]=

1

10

−3

M=10

−3

M

pH=−log10

−3

=3

Explanation:

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Answer 2

Answer:

For HCl, Molarity = Normality (since n-factor is 1)

Number of moles of H

+

=M×V=0.1×10×10

−3

=10

−3

Total volume =10+990ml=1 litre

[H

+

]=

1

10

−3

M=10

−3

M

pH=−log10

−3

=3

Explanation:

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