A 29.00 mL sample of an unknown HClO4 solution requires titration with 23.62 mL of 0.2100 MNaOH to reach the equivalence point. What is the concentration of the unknown HClO4  solution? The neutralization reaction is   HClO4(aq)+NaOH(aq)→H2O(l)+NaClO4(aq) Express your answer using four significant figures.

If 16.0 g of NaOH is added to 0.650 L of 1.00 M Cu(NO₃)₂, how many grams of Cu(OH)₂ will be formed in the following precipitation reaction?2 NaOH(aq) + Cu(NO₃)₂(aq) → Cu(OH)₂ (s) + 2 NaNO₃(aq)

The Borax solution (Na2B4O7) was standardized by titrating 20.00 mL of sample with 1.044 M solution of H2SO4. It takes 2.63 mL of this H2SO4 to reach the end point. What was the concentration of this Borax solution?B4O7 2– (aq) + 7 H2O(l) → 2 B(OH)3(aq) + 2 B(OH)4 – (aq) 2 B(OH)4 – (aq) + H2SO4(aq) → 2 B(OH)3(aq) + 2 H2O(l) + SO4 2– (aq)

Barium sulfate, BaSO4(s), is insoluble in water and can be formed according to the net ionic equation Ba2+(aq) + SO42–(aq) → BaSO4(s) Calculate the volume of 0.500 M K2SO4(aq) solution that is required to precipitate all the barium from 25.0 mL of 0.350 M Ba(NO3)2(aq).

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO₂ (s) + 4 HCl(aq) →MnCl₂(aq) + 2 H₂O(1) + Cl₂(g) How much MnO₂ (s) should be added to excess HCl(aq) to obtain 295 mL Cl₂(g) at 25 °C and 715 Torr? and X la # mass of MnO₂: 3 E D C $ 4 R F 675 % V T G

A titration experiment required 25.08 mL of NaOH, which had a concentration of 0.400 M, to reach the endpoint when titrating 5.00 mL of an H2SO4 sample with an unknown concentration. What is the concentration of the H2SO4 solution in molarity? H2SO4 (aq)+ 2 NaOH (aq)→ Na2SO4(aq) + 2 H20(1)

A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.

A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember, KHP ia potassium hydrogen phthalate, KHC8H4O4, not potassium hydrogen phosphorus).

A 350.0 mL solution of 0.150 M HNO3(aq) is mixed with a solution of 230.0 mL of 0.240 M HCl(aq). How many moles of H+(aq) are present in the final solution? (Both HNO3 and HCl are strong acids).

chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl (aq), as described by the chemical equation MnO2 (s) + 4 HCl (aq) -> MnCl2 (aq) + 2 H2O (l) + Cl2 (g) How much MnO2 (s) should be added to excess HCl (aq) to abtain 145 mL Cl2 (g) at 25 degrees celsius and 735 Torr? Mass of MnO2 = ? g