KMnO4(aq) + 8 HCl(aq) + 5 FeCl2(aq) → MnCl2(aq) + 5 FeCl3(aq) + 4 H2O(l) + KCl(aq) If 28.13 mL of 0.1133 M KMnO4 was added to the solution to reach the end point, what mass of FeCl2 was in the sample?

A 0.450 g sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CaCO3(s) + 2HCl(aq) - CaCl2(aq) + H2O(l) + CO2(g) The excess HCl(aq) is titrated by 5.60 mL of 0.125 M NaOH(aq). Calculate the mass percentage of CaCO3(s) in the sample. mass percentage:

If 785 mL of 0.350 M AgNO₃ is added to 475 mL of 0.250 M CaBr₂, how many moles of AgBr precipitate will be formed? The balanced equation is 2 AgNO₃(aq) + CaBr₂(aq) → 2 AgBr(s) + Ca(NO₃)₂(aq)

Calculate the number of milliliters of 0.779 M KOH required to precipitate all of the Pb²* ions in 122 mL of 0.541 M Pb(NO3)2 solution as Pb(OH)2. The equation for the reaction is: Pb(NO3)2(aq) + 2KOH(aq) –→Pb(OH)2(s) + 2KNO3(aq) mL KOH

+ Titration of Weak Acid with Strong Base A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA (aq) + OH (aq) →A (aq) + H₂O (1) A certain weak acid, HA, with a K, value of 5.61 x 106, is titrated with NaOH. Part A A solution is made by titrating 9.00 mmol (millimoles) of HA and 3.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ▸ View Available Hint(s) pH = Submit Part B pH = VE ΑΣΦ More strong base added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 42.0 mL ? Express the pH numerically to two decimal places. ▸ View Available Hint(s) IV— ΑΣΦ Submit ? 16 of 3 Review | Constants | Periodic

Calculate the number of milliliters of 0.754 M KOH required to precipitate all of the Zn2+ ions in 162 mL of 0.731 M Zn(NO3)2 solution as Zn(OH)2. The equation for the reaction is: Zn(NO3)2(aq) + 2KOH(aq) Zn(OH)2(s) + 2KNO3(aq)

A 15.0 mL of 0.500 M Ba(OH)2 is required to titrate a 10.0 mL of an unknown solution of HNO3, according to the following equation:       Ba(OH)2(aq) + 2HNO3(aq) → Ba(NO3)2(aq + 2H2O(l).  What is the concentration of the HNO3 solution?

A sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required.    The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s)    How many moles of Ag+ (aq) ions are used to reach the end point?    How many moles of Cℓ- (aq) have reacted in the titration?    How many grams of chloride are present in the sample?   What is the mass percent of chloride in the sample?

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 chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 75. mg of oxalic acid (H2C2O4), 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 his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 54.3 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. M ☐ x10