Question

In: Chemistry

Assume you will titrate a sodium carbonate solution with sulfuric acid. All of the following apply...

Assume you will titrate a sodium carbonate solution with sulfuric acid. All of the following apply except:

a.

The end point should coincide with the equivalence point.

b.

Either the mass of sodium carbonate or the molarity of the sulfuric acid must be known initially.

c.

The titration depends on the volume of water added to dissolve the sodium carbonate.

d.

The volume of sulfuric acid added will be carefully measured.

e.

An indicator will be used.

Solutions

Expert Solution


Related Solutions

In an experiment, a solution sulfuric acid is mixed with an excess of sodium carbonate. One...
In an experiment, a solution sulfuric acid is mixed with an excess of sodium carbonate. One of the products is a gas. This gas is collected in a one-liter flask at 20.0°C. What will be the pressure in the flask if 113 mL of the sulfuric acid solution is used? The [H2SO4] can be found from its complete titration (25.0 mL H2SO4) with 16.0 mL of NaOH (NaOH : standardized with 58.7 mL of a 1.000 M HCl)
A solution of sodium hydroxide was neutralized by sulfuric acid. The volume of sodium hydroxide solution...
A solution of sodium hydroxide was neutralized by sulfuric acid. The volume of sodium hydroxide solution used was 675.0 mL, and the concentration was 0.875 M. Calculate the moles of sulfuric acid that were neutralized (assuming that the reaction goes to completion). Give your answer to three significant figures. 2NaOH (aq) + H2SO4 (aq) ? Na2SO4 (aq) + 2H2O (l
how much of 10% sodium carbonate would be needed to bring 1.5mL of Na2SO4 (sulfuric acid)...
how much of 10% sodium carbonate would be needed to bring 1.5mL of Na2SO4 (sulfuric acid) [18M] to a pH of ~8?
4.8 Sodium sulfide reacts with sulfuric acid to produce sodium sulfate and hydrogen sulfide. Assume that...
4.8 Sodium sulfide reacts with sulfuric acid to produce sodium sulfate and hydrogen sulfide. Assume that excess sulfuric acid is allowed to react with 10.0 g of sodium sulfide and calculate: a) the moles of sodium sulfide used. b) the moles of hydrogen sulfide liberated. c) the grams of hydrogen sulfide liberated. d) the volume of hydrogen sulfide liberated at STP. Answer: a)0.128 mole; b) 0.128 mole; c) 4.36 g; d) 2.87 liters
Suppose you add a solution of calcium hydroxide to a solution of sodium carbonate and a...
Suppose you add a solution of calcium hydroxide to a solution of sodium carbonate and a precipitate forms. You measure the total amount of the precipitate (in g) as a function of time. At time 0, 20.0 s, 40.0 s and 60.0 s you get a cumulative weight of 0.00 g, 4.82 g, 6.33 g and 8.49 g of the precipitate, respectively. What is the average rate of reaction between 40 and 60 seconds in mol/s? Enter a numerical value...
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide...
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1799 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 14.33 mL of the standard solution. What...
12. A 15.7-g sample of sodium carbonate is added to a solution of acetic acid weighing...
12. A 15.7-g sample of sodium carbonate is added to a solution of acetic acid weighing 19.4 g. The two substances react, releasing carbon dioxide gas to the atmosphere. After reaction, the contents of the reaction vessel weighs 28.4 g. What is the mass of carbon dioxide given off during the reaction? 13. Cadmium metal reacts vigorously with yellow crystals of sulfur to produce a yellow powder of cadmium sulfide. A chemist determines that 112 g of cadmium reacts with...
The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate...
The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of . In the titration, of the sodium hydroxide solution was required to react with KHP. Calculate the molarity of the sodium hydroxide.
A solution is prepared by dissolving 11.6 g of a mixture of sodium carbonate and sodium...
A solution is prepared by dissolving 11.6 g of a mixture of sodium carbonate and sodium bicarbonate in 1.00 L of water. A 300.0 cm3sample of the solution is then treated with excess HNO3 and boiled to remove all the dissolved gas. A total of 0.940 L of dry CO2 is collected at 298 K and 0.972 atm. 1. Find the molarity of the carbonate in the solution. 2. Find the molarity of the bicarbonate in the solution.
Suppose you take a 35.00 mL sample of this acid solution. You then titrate it with...
Suppose you take a 35.00 mL sample of this acid solution. You then titrate it with a 0.1522 M sodium hydroxide solution. A volume of 39.25 mL of the sodium hydroxide was required to complete the titration. What is the concentration of this unknown hydrochloric acid solution? (shortest and easiest way please)
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT