Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. 0.500 mole of Ca(NO3)2 in 800.0 mL of solution

[Ca²⁺] = 0.625 M

[NO₃⁻] = 1.25 M

Explanation:

Step 1: Calculate the initial molar concentration of calcium nitrate

[Ca(NO₃)₂] = 0.500 mol / 0.8000 L = 0.625 M

Step 2: Write the reaction for the ionization of calcium nitrate

Calcium nitrate is a strong electrolyte that ionizes according to the following equation.

Ca(NO₃)₂(aq) ⇒ Ca²⁺(aq) + 2 NO₃⁻(aq)

Step 3: Calculate the concentrations of the ions

The molar ratio of Ca(NO₃)₂ to Ca²⁺ is 1:1. The concentration of Ca²⁺ is 1/1 × 0.625 M = 0.625 M.

The molar ratio of Ca(NO₃)₂ to NO₃⁻ is 1:2. The concentration of Ca²⁺ is 2/1 × 0.625 M = 1.25 M.

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer