Question

A 1.294-g sample of a metal carbonate (MCO₃) is reacted with 500 mL of a 0.100 M HCl solution. The excess HCl acid is then neutralized by 32.80 mL of 0.588 M NaOH. Identify M.

Answer 1

To identify the metal (M) in the metal carbonate (MCO₃), we need to use stoichiometry and mole ratios from the balanced equation. By calculating the number of moles of HCl used and the number of moles of MCO₃, we can determine the molar mass of M and identify the metal.

Step-by-step explanation:

To identify the metal (M) in the metal carbonate (MCO₃), we need to use stoichiometry and mole ratios from the balanced equation. The balanced equation for the reaction between the metal carbonate and hydrochloric acid (HCl) is:

MCO₃ + 2HCl → MCl₂ + CO₂ + H₂O

From the equation, we can see that 1 mole of MCO₃ reacts with 2 moles of HCl. First, we calculate the number of moles of HCl used:

Moles of HCl = volume of HCl solution (L) × concentration of HCl (mol/L)

Next, we use the mole ratio to determine the number of moles of MCO₃. Since we have the mass of the sample, we can convert it to moles:

Moles of MCO₃ = mass of sample (g) / molar mass of MCO₃ (g/mol)

Once we have the number of moles of MCO₃, we can calculate the molar mass of M:

Molar mass of M = mass of MCO₃ (g) / moles of MCO₃ (mol)

By substituting the given values into the equations, we can solve for the molar mass of M and identify the metal.