Ask a New Question

A sample of conc. nitric acid has a density of 1.41g/ml and contains 70% HNO3 by mass.

What mass of HNO3 is present per L of solution?
What is the molarity?

3 answers

Assume 1 liter. then mass of acid is .7*1.41*1000, and from that calculate moles acid
Volume is 1liter,

molarity=molesacid/1

s12

.987 g HNO3

M=.0157

Ask a New Question or answer this question.

Similar Questions

A commercial sample of concentrated aqueous nitric acid (HNO3) is 18.2% nitric acid base mass and has a density of 1.12 g/mL.(a)
1. 3 answers
Hi,there was an error with the procedure. 1.0g NaOH sample was dissolved in 5ml of water and acidified with 4ml of conc. nitric
1. 0 answers
Given 50 ml of concentrated nitric acid.The density of the concentrated acid is 1.42 g/ml and is 70% HNO3 by wt. Calc. the
1. 1 answer
Given 50 ml of concentrated nitric acid.The density of the concentrated acid is 1.42 g/ml and is 70% HNO3 by wt. Calc. the
1. 1 answer

more similar questions