# CHEMISTRY

A solution of H2SO4(aq) with a molal concentration of 1.94m has a density of 1.119g/mL. What is the molar concentration of this solution?

My work:
So Molar concentration = molal concentration * density
= 1.94 mol/kg * 1.119 kg/L = 2.17 M

1. 👍 0
2. 👎 1
3. 👁 1,832
1. Your error is that molar concn x density is NOT molality.

m = moles/kg solvet = 1.94 mol/kg solvent
How much is 1.94 moles H2SO4? That is M x L = 1.94 x 98 = about 190g (remember that's 1.94 mols).
It was dissolve in 1 kg solvent which is 1000 g. It had 190 g (approximate) H2SO4 for a total mass of 1000 +190 = 1190.
mass = volume x density or
volume = 1190 g/1.119 = about 1060 mL or 1.060 L.
So M = moles/L = 1.94 mol/1.063 L = about 1.8 M. You clean up the figures but 1.8 is close to the right answer.

1. 👍 0
2. 👎 3
2. Thanks so much! :] I understand my mistake!

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chemistry

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)? A) 0.40 M B) 0.10 M C) 0.20 M D) 0.25 M E) 0.36 M The answer is

2. ### Chem

A solution of H2SO4(aq) with a molal concentration of 8.01 m has a density of 1.354 g/mL. What is the molar concentration of this solution?

3. ### AP Chemistry

An aqueous sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution at 20°C has a density of 1.3294 g/mL. Calculate (a) the molarity, (b) the molality, (c) the percent by mass, and (d) the mole fraction of H2SO4

4. ### chemistry h/w help

The concentration of lead nitrate (Pb(NO3 )2 ) in a 0.726 M solution is __________ molal. The density of the solution is 1.202 g/mL.

1. ### Chemistry:Important!!!!!!!

20.00 mL of a H2SO4 solution with an unknown concentration was titrated to a phenolphthalein endpoint with 39.13 mL of a 0.1061 M NaOH solution. What is the concentration of the H2SO4 solution?

2. ### Chemistry

Write the balanced neutralization reaction between H2SO4 and KOH in aq. solution. .350 L of .410 M H2SO4 is mixed with .300 L of .230 M KOH. What concentration of sulfuric acid remains after neutralization? ______ M H2SO4

3. ### AP Chem

It takes 58 mL of 0.124 M KOH to neutralize 34.5 mL of H2SO4 solution. What is the concentration of the H2SO4 solution? Answer in unites of moles/liter.

4. ### chemistry

The density of 2 molal aqueous solution of NaOH is 1.10gm/L. Calculate the molarity of the solution.

1. ### chemistry 112

A volume of 60.0mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 19.2mL of 1.50 M H2SO4 was needed? The equation is

2. ### Chemisty

A 25-mL sample of 0.160M solution of NaOH is titrated with 17 mL of an unknown solution of H2SO4. What is the molarity of the sulfuric acid solution? A. 0.004M H2SO4 B. 0.235M H2SO4 C. 0.117M H2SO4 D. 0.002M H2SO4

3. ### Chemistry

A solution of H2SO4(aq) with a molal concentration of 1.66 m has a density of 1.104 g/mL. What is the molar concentration of this solution?

4. ### Chemistry

Concentrated sulfuric acid is 18.4 molar and has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar the solution has a density of 1.38 grams per milliliter. This concentration of H2SO4 is often used in