Question

9. What is the hydroxide-ion concentration in a solution formed by combining 200. mL of 0.16 M HCl with 300. mL of 0.091 M NaOH at 25°C? HCl(aq) + NaOH(aq) ? NaCl(aq) + H2O(l) 10. What is the pH of a solution prepared by dissolving 0.241 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 2.00 L? (R = 0.0821 L · atm/(K · mol)) (Use gas law equation to calculate Mole of HCl dissolved in 2.00 L of water, Calculate M/L followed by using equation of ionic product (Kw = 1 x 10-14) to calculate [H3O+]. 11. A 20.27 g of unknown metal carbonate (MCO3) is dissolved in 500 ml of a 1.00 M HCl. The excess acid is then neutralized by 32.08 ml of 0.588 M NaOH. Identify M. (Hint: Find the molar mass of the MCO3 then subtract it from mass of CO32-.) 12. A 2.500 G sample of mixture of Na2CO3 and NaCl is dissolved in 25.0 ml of 0.798 M HCl. Some acid remains after the treatment of the sample. (a). Write the net ionic equation for the reaction of sodium carbonate with HCl acid. (b). If 28.7 ml of 0.108 M NaOH were required to titrate the excess HCl, how many moles of Na2CO3 were present in the original sample? (c) What is the % of Na2CO3 in original sample?

          9. What is the hydroxide-ion concentration in a solution formed by combining 200. mL of 0.16 M HCl with 300. mL of 0.091 M NaOH at 25°C?
HCl(aq) + NaOH(aq) ? NaCl(aq) + H2O(l)
10. What is the pH of a solution prepared by dissolving 0.241 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 2.00 L? (R = 0.0821 L · atm/(K · mol))
(Use gas law equation to calculate Mole of HCl dissolved in 2.00 L of water, Calculate M/L followed by using equation of ionic product (Kw = 1 x 10-14) to calculate [H3O+].
11. A 20.27 g of unknown metal carbonate (MCO3) is dissolved in 500 ml of a 1.00 M HCl. The excess acid is then neutralized by 32.08 ml of 0.588 M NaOH. Identify M. (Hint: Find the molar mass of the MCO3 then subtract it from mass of CO32-.)
12. A 2.500 G sample of mixture of Na2CO3 and NaCl is dissolved in 25.0 ml of 0.798 M HCl.
Some acid remains after the treatment of the sample.
(a). Write the net ionic equation for the reaction of sodium carbonate with HCl acid.
(b). If 28.7 ml of 0.108 M NaOH were required to titrate the excess HCl, how many moles of Na2CO3 were present in the original sample?
(c) What is the % of Na2CO3 in original sample?

9. What is the hydroxide-ion concentration in a solution formed by combining 200. mL of 0.16 M HCl with 300. mL of 0.091 M NaOH at 25°C?
HCl(aq) + NaOH(aq) ? NaCl(aq) + H2O(l)
10. What is the pH of a solution prepared by dissolving 0.241 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 2.00 L? (R = 0.0821 L · atm/(K · mol))
(Use gas law equation to calculate Mole of HCl dissolved in 2.00 L of water, Calculate M/L followed by using equation of ionic product (Kw = 1 x 10-14) to calculate [H3O+].
11. A 20.27 g of unknown metal carbonate (MCO3) is dissolved in 500 ml of a 1.00 M HCl. The excess acid is then neutralized by 32.08 ml of 0.588 M NaOH. Identify M. (Hint: Find the molar mass of the MCO3 then subtract it from mass of CO32-.)
12. A 2.500 G sample of mixture of Na2CO3 and NaCl is dissolved in 25.0 ml of 0.798 M HCl.
Some acid remains after the treatment of the sample.
(a). Write the net ionic equation for the reaction of sodium carbonate with HCl acid.
(b). If 28.7 ml of 0.108 M NaOH were required to titrate the excess HCl, how many moles of Na2CO3 were present in the original sample?
(c) What is the % of Na2CO3 in original sample?

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