Posted by **Connie** on Thursday, April 28, 2011 at 11:37am.

calculate the volume(ml) of a 0.215M KOH solution that will completely neutralize each of the following?

a) 2.50ml of a 0.825M H2SO4 solution

b) 18.5ml of a 0.560 M HNO3 solution

c) 5.00mL of a 3.18 M H2SO4 solution

- chemistry -
**DrBob222**, Thursday, April 28, 2011 at 1:10pm
All of these are done the same way.

1. Write and balance the equation.

2KOH + H2SO4 ==> K2SO4

2. Calculate moles. moles = M x L.

moles H2SO4 = M x L = 0.825 x 0.0025 L = 0.00206

3. Using the coefficients in the balanced equation, convert moles H2SO4 to moles KOH.

0.00206 moles H2SO4 x (2 moles KOH/1 mol H2SO4) = 0.00206 x 2 = 0.00413 moles KOH.

4. Then M KOH = moles KOH/L KOH. We know M and moles, solve for L.

0.215M = 0.00413/L

L = 0.00413/0.215 = 0.01919 L or 19.19 mL which rounds to 19.2 mL to three significant figures.

## Answer this Question

## Related Questions

- chemistry - 35.00mL of 0.250M KOH solution is required to completely neutralize ...
- Chemistry - Calculate the volume of 2.00 M solution of KOH that is required to ...
- Chemistry - Calculate the volume of 2.00 M solution of KOH that is required to ...
- chemistry - A 27.00mL sample of an H2SO4 solution of unknown concentration is ...
- Chemistry - A 25.00-mL sample of an H2SO4 (2 and 4 are subscripted) solution of ...
- Chemistry - A 25.00-mL sample of an H2SO4 (2 and 4 are subscripted) solution of ...
- Chem - 1. What is the molarity of a copper(II) dihydroxide [Cu(OH)2] solution if...
- Chemistry - A volume of 60.0 of aqueous potassium hydroxide (KOH) was titrated ...
- chemistry - 1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of ...
- Chemistry - Given one of the following solution: 50.00mL of 0.10M of K2CrO4 ...