# Chemistry

posted by .

Calculate the pH and the pOH of an aqueous solution that is 0.025 M in HCl(aq) and 0.075 M in HBr(aq) at 25°C.

• Chemistry -

extremely easy. Sorry! pH=1 and pOH = 13

• Chemistry -

Nope. Tricky question.
Suppose you take 1 L of each. That gives you 1 L x 0.025 mol/L HCl = 0.025 mols.

1L x 0.075 mol/L HBr = 0.075 mols.
Total mols = 0.025+0.075 = 0.1 mol but what's the volume? The volume is 2L so
M = 0.1 mol/2.0L = 0.05 M for H^+. Take pH and pOH from that. I get about 1.3 and 12.7.

## Similar Questions

1. ### Chemistry

calculate the pH and the pOH of an aqueous solution that is 0.035 M In HCI and 0.080 M in HBr?
2. ### Chemistry

Complete this table of values for four aqueous solutions at 25 °C. Solution A: [H+]=0.0093M [OH-]=?
3. ### Chemistry

A 100.0mL solution containing aqueous HCl and HBr was titrated with 0.1290M NaOH. The volume of base required to neutralize the acid was 47.56mL. Aqueous AgNO3 was then added to precipitate the Cl- and Br- ions as AgCl and AgBr. The …
4. ### Chemistry

Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
5. ### Chemistry

Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
6. ### Chemistry

Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
7. ### Chemistry

Calculate the Ph and POH of an aqueous soltuion that is 0.500 M in HCl(aq) and 0.085 M in HBr (aq) at 25 degrees C.
8. ### Chemistry 2

Calcualte PH and POh of an aqueous solution that is 0.050 M in HCL and 0.085 M in HBr at 25 degrees C
9. ### chemistry

Calculate the PH and POH of an aqueous solution that is 25.00% of HCL by mass and density of 1.35g/no
10. ### chemistry

Calculate the PH and POH of an aqueous solution that is 25.00% of HCL by mass and density of 1.35g/ml

More Similar Questions