Posted by **anonymous** on Sunday, April 11, 2010 at 6:19am.

Two aqueous solutions are mixed: 50.0 mL of 1.60×10−2 M H2SO4 and 50.0 mL of 3.75×10−2 M NaOH.

what is the PH of the following solution?

- chemistry -
**DrBob222**, Sunday, April 11, 2010 at 1:40pm
The trick to these question is to recognize what you have in the final solution.

Write the equation.

H2SO4 + 2NaOH ==> Na2SO4 + 2H2O

moles H2SO4 = M x L = ??

moles NaOH = M x L= ??

moles H2SO4 required to use all of it will be moles H2SO4 x 2 (since there are two moles NaOH for every mole of H2SO4). Look at those numbers, see which is in excess and use that to calculate either the OH or the H depending upon the one in excess.

Post your work if you get stuck.

- chemistry -
**Anonymous**, Thursday, July 11, 2013 at 7:39am
so what the h is the answer

## Answer this Question

## Related Questions

Chemistry - Consider the following reaction: PbCl2 + 2 NaOH -> Pb(OH)2 + 2 ...

Chemistry - Which one of the following pairs of 0.100 mol L-1 solutions, when ...

Finite Math - Solve the system of linear equations, using the Gauss-Jordan ...

biology - Given the part of the molecule shown below, can the underlined atom ...

CHEMISTRY - Suppose that you have 0.500 L of each of the following solutions, ...

CHEMISTRY - 1. Suppose that you have 0.500 L of each of the following solutions...

CHEMISTRY - 1. Suppose that you have 0.500 L of each of the following solutions...

Grade 12 Calculus - Evaluate each of the following. Show all your calculations...

calculus (gr 12) - Evaluate each of the following. Show all your calculations. a...

calculus (gr 12) - Evaluate each of the following. Show all your calculations. a...