0.4556 g of Na2CO3 (FW = 105.99 g/mol) was dissolved in water and titrated with a solution H2SO4 of unknown Normality.
20.35 mL of H2SO4 solution was required to reach the final endpoint. What is the Normality of the H2SO4 solution?
(Answer in 4 sig figs)
0.4556 g of Na2CO3 (FW = 105.99 g/mol) was dissolved in water and titrated with a...
4.00 g Na2CO3 is dissolved in H2O and titrated with HCl. 48.0 mL of a HCl solution were required to titrate the Na2CO3 solution. What is molarity of HCl solution? Na2CO3(aq) + 2HCl(aq) --> 2NaCl(aq) + H2O(l) + CO2(g)
A 22.9 % (by mass) solution of ferrocene (FW = 186.04 g/mol) dissolved in hexane (FW = 86.18 g/mol) has a density of 1.421 g/mL. What is the mole fraction (Χ) of ferrocene? Ferrocene is a non-electrolyte.
A sample may contain Na2CO3 (105.989 g/mol), NaHCO3 (84.007 g/mol), NaOH (39.977 g/mol) or a compatible mixture of these bases. A 0.8412-g sample titrated directly to the methyl orange endpoint required 45.38 mL of 0.1320 M HCl. Another 0.8412-g sample was titrated to the phenolphthalein endpoint with the same acid. It required 28.32 mL acid. (a) What base(s) are present in the sample? (b) What is/are the percentage(s) of the base(s) in the sample?
A solid weak acid is weighed, dissolved in water and diluted to exactly 50.00 ml. 25.00 ml of the solution is taken out and is titrated to a neutral endpoint with 0.10 M NaOH. The titrated portion is then mixed with the remaining untitrated portion and the pH of the mixture is measured. Mass of acid weighed out (grams) 0.773 Volume of NaOH required to reach endpoint: (ml) 19.0 pH of the mixture Ihalf neutralized solution 3.54 Calculate the following...
4.00 g Na2CO3 is dissolved in H20 and titrated with HCI. 48.0 mL of a HCl solution were required to titrate the Na2CO3 solution. What is molarity of HCl solution? Na2CO3(aq) + 2HCl(aq) --> 2NaCl(aq) + H2O(l) + CO2(g) O 1.88 molar O 3.21 molar O 1.57 molar O 9.37 molar O 2.59 molar O 0.123 molar 0.553 molar 02.02 molar
7. A small amount of CuSO4*5H20 (0.973 g) was dissolved in 100.0 mL of water, When a 10.0 mL aliquot was titrated with EDTA, the endpoint was reached at 38.05 mL. A 10.0 mL aliquot of a 100.00 mL sample of unknown copper solution was also titrated with the same solution of EDTA. The endpoint was reached at 35.23 mL. What is the mass of Cu?' in the unknown solution?
A Na2CO3(MM = 105.99 G/MOL) standard solution is prepared by transferring 2.4814 grams of primary standard-grade sodium carbonate to 250.0mL volumetric flask, dissolving the sample in about 100 mL of distilled deionized water and diluted to the mark. A 25.00mL aliquot is taken and titrated with 40.18mL of HCl solution. Calculate the concentration of the HCl solution.
An aqueous ethylene glycol (HOCH2CH2OH, FW=62.07 g/mol) solution with a mass of 220.7 mg is titrated with 45.3 mL of 0.0671 M Ce4 in 4 M HClO4. The solution is held at 60 °C for 15 min to oxidize the ethylene glycol to formic acid (HCO2H) and carbon dioxide. The excess Ce4+ is titrated with 11.73mL of 0.0449 M Fe2+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution? mass percent =__________%
An aqueous ethylene glycol (HOCH2CH2OH, FW = 62.07 g/mol) solution with a mass of 253.1 mg is titrated with 49.5 mL of 0.0895 M Ce4+ in 4 M HCIO4. The solution is held at 60°C for 15 minutes to oxidize the ethylene glycol to formic acid (HCO2H) and carbon dioxide. The excess Ce4+ is titrated with 10.81 mL of 0.0439 M Fe2+ to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution? Number
A sample of sodium carbonate (Na2CO3 (s), 105.99 g/mol) with a mass of 0.3531 g is titrated with 0.042 L HCl (aq). Calculate the molarity of the HCl solution.