Question

How many mL of 0.563 M HNO3 are needed to dissolve 7.83 g of BaCoz? 2HNO3(aq) + BaCO3(s) — Ba(NO3)2(aq) + H2O(1) + CO2(8) mL

Answer 1

Volume of HNO₃ required = 140 mL

Step-by-step explanation:

Given data:

Molarity of HNO₃ = 0.563 M

mass of BaCO₃ = 7.83 g

Volume of HNO₃ = ?

Solution:

First of all we will write the balance chemical equation

2HNO₃ + BaCO₃ → Ba(NO₃)₂ + H₂O + CO₂

Number of moles of BaCO₃ = mass / molar mass

Number of moles of BaCO₃ = 7.83 g / 197.34 g/mol

Number of moles of BaCO₃ = 0.04 mol

Now we compare the moles of BaCO₃ and HNO₃ .

BaCO₃ : HNO₃

1 : 2

0.04 : 2×0.04 = 0.08 mol

Volume of HNO₃ required = number of moles / Molarity

Volume of HNO₃ required = 0.08 mol / 0.563 mol/L

Volume of HNO₃ required = 0.14 L

0.14 × 1000 = 140 mL