NaCl is purified by adding HCl to a saturated solution of NaCl (317 g/L). Will pure NaCl precipitate when 10mL of 13.0 M HCl is added to 0.2 L of saturated solution?

Yes, pure NaCl will precipitate out of the solution

Explanation:

The parameters of the NaCl solution and HCl mixture are;

The saturation of the NaCl solution = Saturated solution

The mass concentration of the NaCl solution = 317 g/L

The volume of the HCl added = 10 mL

The concentration of the HCl added = 13.0 M HCl

The volume of the saturated NaCl solution = 0.2 L

The molar mass of NaCl = 58.44 g/mol

The number of moles of NaCl per liter = (317 g/L)/(58.44 g/mol) = 7925/1461 moles ≈ 5.42 moles

The ionization of the molecules in solution are;

HCl (aq) + H₂O (l) → H₃O⁺ (aq) + Cl⁻ (aq)

NaCl (s) ↔ Na⁺ (aq) + Cl⁻ (aq)

The number of moles of the Cl⁻ ion from the HCl is 13 moles per liter, the number of moles of Cl⁻ ion from the saturated solution of NaCl is approximately 5.42 moles, therefore, ionic product I.P. of the solution of Cl⁻ ions is larger than the solubility product of the solution, of the NaCl and according to Le C h a t e l i e r's principle, NaCl will precipitate out of the solution

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

the answer is 1260

you spend 7 hours in school for 1 school day with 5 school days in 1 school week with 36 school weeks in a school year.

7*5*36= 1260 it's all about multiplying