HA and HB are two strong monobasic acids. 25.0cm3 of 6.0mol/dm3 HA is mixed with 45.0cm3 of 3.0mol/dm3 HB.

What is the H+ (aq) concentration in mol/dm3 in the resulting solution ?

A 1.9

B 2.1

C 4.1

D 4.5

If anyone could explain how to reach an answer that would be so helpful !!

The H+ (aq) concentration of the resulting solution is 4.1 mol/dm³

(Option C)

Explanation:

Given;

concentration of HA, = 6.0mol/dm³

volume of HA,  = 25.0cm³, = 0.025dm³

Concentration of HB, = 3.0mol/dm³

volume of HB, = 45.0cm³ = 0.045dm³

To determine the H+ (aq) concentration in mol/dm³ in the resulting solution, we apply concentration formula;

where;

is initial concentration

is initial volume

is final concentration of the solution

is final volume of the solution

Therefore, the H+ (aq) concentration of the resulting solution is 4.1 mol/dm³

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%