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Calculate the pH of a solution formed by mixing 10.0 mL of 0.100 M HBr with 20.00 mL of 0.200 M HCL.

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Hubert Koch
Hubert KochLv2
29 Sep 2019

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Related questions

Consider a solution formed by mixing

50.0 mL of 0.100 M H2SO4,

30.0 mL of 0.1000 M HOCl,

25.0 mL of 0.200 M NaOH,

25.0 mL 0.100 M Ba(OH)2, and

10.0 mL of 0.150 M KOH.

Calculte the pH of this solution.

Ka (HOCl) = 3.5 x 10-8

What is the pH?

1) Calculate of pH of each of the following strong acid solutions:

(a) 8.5 x 10-3 M HBr

(b) 1.52 g of HNO3 in 575 mL of solution

(c) 5.00 mL of 0.250 M HClO4 diluted to 50.0 mL

(d) a solution formed by mixing 10.0 mL of 0.100 M HBr with 20.0 mL of 0.200 M HCl.

 

2) Calculate [OH-] and pH for

(a) 1.5 x 10-3 M Sr(OH)2

(b) 2.250 g of LiOH in 250.0 mL of solution

(c) 1.00 mL of 0.175 M NaOH diluted to 2.00 L,

(d) a solution formed by adding 5.00 mL of 0.105 M KOH to 15.0 mL of 9.5 x 10-2 M Ca(OH)2

 

3) Latic acid (CH3CH(OH)COOH) has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44. Calculate Ka.

 

4) A 0.100 M solution of chloroacetic acid (ClCH2COOH) is 11.0% ionized. Using this information, calculate [ClCH2COO-], [H+], [ClCH2COOH], and Ka for chloroancetic acid.

A 50.0 mL solution of 0.200 M ammonia (pKa of ammonia is 9.24) is titrated by 0.100 M HCl. Calculate the pH of the solution when, A.) the volume of HCl is 20.00 mL B.) the volume of HCl is 100.0 mL

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