Question

An
aqueous solution that is 16 percent sulfuric acid (H2SO4) by mass
has a density of 1.109 g/mL at 25°C. Determine (a) the molarity and
(b) the molality of the solution at 25°C.

Answer #1

The concentrated sulfuric acid we use in the laboratory is 97.8
percent H2SO4 by mass. Calculate the molality and molarity of the
acid solution. The density of the solution is 1.83 g/mL.

What is the molal and molarity concentration of a 98.0 mass
percent aqueous sulfuric acid solution. The density of the solution
is 1.83 g/mL.

Calculate the Molality of 3.75 M H2SO4(aq), sulfuric acid
solution which has a density of 1.230 g/ml

Concentrated H2SO4 (sulfuric acid) is 97% by mass and has a
density of 1.84g/mL. What is its molarity?

An old sample of concentrated sulfuric acid to be used in the
laboratory is approximately 97.3 percent H2SO4 by mass. Calculate
the molality and molarity of the acid solution. The density of the
solution is 1.83 g/mL.
m
M

The lead storage batteries used in automobiles have a sulfuric
acid (H2SO4) concentration of 3.75 M. The density of the sulfuric
acid solution is 1.230 g/mL and the molar mass of sulfuric acid is
98.08 g/mol. What is molality of sulfuric acid?

Determine the molarity and molality of an aqueous concentrated
hydrochloric acid solution that is 33% by mass acid with a density
= 1.33 g/mL

Nitric acid is usually available in a concentrated form of 70.3%
by mass aqueous solution with a density of 1.41 g/mL. Calculate the
molarity and molality of this solution.

An aqueous solution is 8.00% ammonium chloride, NH4Cl, by mass.
The density of the solution is 1.023 g/mL. What are the molality,
mole fraction, and molarity of NH4Cl in the solution?

Commercially prepared concentrated HCl is an aqueous solution
that is 37.1% by mass HCl and has a density of 1.18 g/mL. (Water is
the solvent). Determine the molarity and molality of HCl in this
solution.

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