A student mixed the following reactants, using the general procedure for the experiment: 13.07 mL of 0.1000M KI, 20.58 mL of 0.001000 M Na2SO3, 12.44 mL of 0.04000M KBrO3, and 13.83 mL of 0.1000M HCl.  Calculate the concentration of H+ in the mixture after all of the solutions have been combined

A student mixed the following reactants, using the general procedure for the experiment: 12.53 mL of 0.1000M KI, 18.4 mL of 0.001000 M Na2SO3, 11.86 mL of 0.04000M KBrO3, and 12.2 mL of 0.1000M HCl. Calculate the concentration of H+ in the mixture after all of the solutions have been combined

A solution contains Cr3+ and Mg2+. The addition of 1.00 L of 1.51 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 50.1 g . Find the mass of Cr3+ in the original solution.

A student determined the concentration of copper by ion exchange. He obtained the following results: 28.61 mL of 0.0810 M NaOH solution was required to titrate the eluate (HCl solution) from the column. He used 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of H+ present in the eluate.

The molar mass of a metal carbonate can be determined by adding an excess of HCl to completely react with the carbonate and then “back –titrating” the excess acid with NaOH. If 20.0 mL of 0.0800 M HCl was added to a 0.1022 g sample of MCO3, the excess HCl required 5.64 mL of 0.1000 M NaOH for neutralization. Find the molar mass of MCO3 and identify M.

A student mixed the following reactants, using the general procedure for the experiment: 12.73 mL of 0.1000M KI, 23.77 mL of 0.001000 M Na2SO3, 11.84 mL of 0.04000M KBrO3, and 14.2 mL of 0.1000M HCl.  Calculate the concentration of H+ in the mixture after all of the solutions have been combined

The molarity of an aqueous solution of hydrobromic acid, HBr, is determined by titration with a 0.154 M sodium hydroxide, NaOH, solution. [Review Topics] [References] Use the References to access important values if needed for this question. HBr + NaOH → NaBr + H2O If 35.8 mL of sodium hydroxide are required to neutralize 20.7 mL of the acid, what is the molarity of the hydrobromic acid solution? Molarity M = Submit Answer Retry Entire Group 4 more group attempts remaining Previous

The concentration of an unknown sample of sulfuric acid was determined by the method used in this experiment. In the first titration, the sodium hydroxide was standardized by titrating 0.1852g of oxalic acid dihydrate (molar mass = 126.07g/mol) with 32.30 mL of sodium hydroxide solution. In the second titration, 10.00mL of the unknown sulfuric acid solution was titrated with 12.85mL of the sodium hydroxide solution. What was the concentration of the sulfuric acid?

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 17. mg of oxalic acid (H,C,0,), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 16.4 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. Submit Ass Continue O 2021 McGraw Hill LLC. Al Rights Reserved. Terms of Use I Privacy Center LL

2.0 g of a mixture containing unknown amounts of sodium carbonate, sodium bicarbonate and a neutral component were titrated according to the experimental procedure. Answer the questions that follow related to the individual steps of the titration. Calculate the number of moles of sodium bicarbonate titrated in the second step of the titration if 13.7 ml of 1.0 M HCl were used to titrate the resulting mixture from the first step of the titration with methyl orange as the indicator. Enter your numerical answer below in units of moles with the correct number of significant figures.