A 6.00% NaOH solution by mass has a density of 1.054 g/mL. What is the minimum molarity of an HCl(aq) solution

Question

A 6.00% NaOH solution by mass has a density of 1.054 g/mL. What is the minimum molarity of an HCl(aq) solution that can be used to titrate a 2.00 mL sample of the NaOH(aq) if the titration is to be accomplished without having to refill a 50.00 mL buret used in the titration?

Answer 1

Density of 1.054 g/mL <==> 1054g/L <==> 6.00% NaOH is 63.24g NaOH <==> 1.581 M NaOH
2.00*1.581 <= 50.00*[HCl]
Therefore [HCl] >= 2.00*1.581/50.00 = 0.0632 M
The minimum molarity of the HCl(aq) solution required is 0.0632 M.

Answer 2

Mass 28 g density= .90 g/mL density=mass/volume or, volume=mass/density=28g/0.90g/ml =31.11ml no. of mole=31.11/mw of Nh3 =31.11/17 = 1.83M molarity of solution= 1.83M/l ( 1litre solution) M=mole/volume