1 A solution contains 2.45 g H SOs in 1 liter of water a) What is the pH of the

Question

1 A solution contains 2.45 g H SOs in 1 liter of water a) What is the pH of the solution? b) What mass of Na CO, is required to neutralize the acid? 2 A groundwater is in equilibrium with gases at 1 atm containing 3% by volume CO2. If the bicarbonate concentration is 10° moles per liter, what is the pH? 3 Calculate the pH of waters having the following compositions a) 0.2 g/L of CaO b) 60 mg/L of bicarbonate and 10 M carbon dioxide. c) 0.3 g/L HCI 4 Convert the following concentrations into mgL as CaCO a) Ca2+ 95 mg/L b) Mg-87 mg/L e) Na 125 mg/L d) MgSO4 420 mg/L e) Ca(HCOs)h-221 mg/L 5 Perform an ionic balance on a solution that contains the following compounds. Ca2+ = 94 mg/L Mg2 24 mg/L Na-14 mg/L SO42-=67 mg L CT-24 mg/L HCO3 317 mg/L

Explanation / Answer

Ans 1

Moles of H2SO4 = mass/molecular weight

= 2.45g / 98g/mol

= 0.025 mol

Volume of water V = 1 L

Part a

Concentration of H2SO4 = moles/Volume

= 0.025 mol/L

H2SO4 = 2H+ + SO4 2-

Concentration of H+ = 2 x 0.025 = 0.05 M

pH = - log [H+] = - log (0.05)

= 1.30

Part b

The balanced reaction

H2SO4 + Na2CO3 = Na2SO4 + H2O + CO2

Moles of Na2CO3 required = moles of H2SO4

= 0.025 mol

Mass of Na2CO3 required = moles x molecular weight

= 0.025 mol x 106 g/mol

= 2.65 g

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