1. 90.0 mL of distilled water is added to a 10.0mL sample of 0.150mol/L sodium
chloride. The resulting solution can be described as more
a. dilute
b. concentrated
c. Acidic
d. basic

dilute

Explanation:

A concentrated solution which is used to prepare solutions of lower concentrations by diluting it with addition of water.

A dilute solution is one which contains lower concentration.

Using Molarity equation:

=concentration of stock solution = 0.150 mol/L

= volume of stock solution = 10.0 ml

= concentration of dilute solution = ?

= volume of dilute solution = (10.0+90.0) ml = 100.0 ml

As the concentration is less than the original concentration, the solution is termed as dilute.

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%

answer: -

reaction:

na + cl ⇌ nacl

balanced chemical equation:

na + 2cl ⇌ nacl2

sodium + clorine goes to form sodium chloride (table salt).

the product is nacl2.

and the reactants are na and cl.

(note: if you don’t know what ⇌ means, read below: -

⇌(double head arrow) means reversible reaction).