# Chemistry

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.

1. 👍 0
2. 👎 0
3. 👁 856
1. extremely easy. Sorry! pH=1 and pOH = 13

1. 👍 0
2. 👎 0
posted by Alex
2. 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.

1. 👍 0
2. 👎 0
posted by DrBob222

## Similar Questions

1. ### chemistry

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

asked by okore on October 9, 2017
2. ### chemistry

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

asked by okore on October 9, 2017
3. ### Chemistry

Complete this table of values for four aqueous solutions at 25 °C. Solution A: [H+]=0.0093M [OH-]=? pH=? pOH=? Solution B: [H+]=?[OH-]=1.4e-6M pH=? pOH=? Solution C: [H+]=?[OH-]=? pH=5.36 pOH=? Solution D: [H+]=?[OH-]=? pH=?

asked by Help on October 20, 2011
4. ### Chemistry

Complete this table of values for four aqueous solutions at 25 °C. Solution A: [H+]=0.0093M [OH-]=? pH=? pOH=? Solution B: [H+]=?[OH-]=1.4e-6M pH=? pOH=? Solution C: [H+]=?[OH-]=? pH=5.36 pOH=? Solution D: [H+]=?[OH-]=? pH=?

asked by Help on October 20, 2011
5. ### Chemistry

Each value below represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. pH=9.72 pOH=4.69 pOH=13.62 [H+]=7.5e-2 [H+]=7.8e-9 [H+]=1e-7 [OH-]=4.5e-12 [OH-]=3.5e-5 pH=4.09 pOH=7

asked by Niloo on October 20, 2011
6. ### 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

asked by Jason on February 21, 2014
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.

asked by Help on February 20, 2014
8. ### chemistry

Calculate the pH and pOH of each of the following aqueous solutions of strong acd or base: (a) 0.010 M HNO3(aq) (b) ) 1.0 x 10-3M Ba(OH)2(aq) (c) 10.0 mL of 0.22M KOH(aq) after dilution to 250 mL (d) 100 mL aqueous solution

asked by imelda on September 16, 2014
9. ### Science

How much sodium hydroxide, at what concentration, do I need to add to 500 mL of 0.1 N HCL to obtain pH 6.8. How do you calculate this? pH = -log(H^+) M HCl = N HCl mols = M x L. After you know mols HCl you have, then make a

asked by Ruby on February 5, 2007
10. ### CHEMISTRY- boiling point

0.1m aqueous solution of HCl and 0.1m aqueous solution of C6H12O6. calculate the boiling point of each i know the eq. dTb=Kbm but i have no temperatures. this is the question

asked by lulu78 on October 15, 2010

More Similar Questions