The concentration of borax (Na2B4O5(OH)4) in aqueous solution can be determined through titration with HCI as titrant. The net ionic equation for the titration reaction is: B4O5(OH)42 (aq) + 2 H*(aq) + 3 H₂O <-> 4 H3BO3(aq) In an experiment, a student titrated 5.0 mL borax solution with 5.43 0.249 M HCI solution. Determine the concentration of borax in mol/L. For a strong electrolyte compound with formula X3Y2, if the concentration of cation X is 0.614 M, find the concentration of anion Y in mol/L. The molar solubility of a compound AX₂ is 3.8 x 103 M. Calculate the value of natural log of Ksp (Inksp) for AX₂.

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 316.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 her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 93.2mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.

A 30.00-mL volume of aqueous sulfuric acid, H2SO4, is titrated using 0.200 M NaOH and an indicator that turns color only after all the sulfuric acid protons have reacted with OH- ions. The solution turns color when 48.32 mL of base has been added. What is the molar concentration of the sulfuric acid?

A 0.450 g sample of impure CaCO,(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CACO, (s) + 2 HCI(aq) CaCl, (aq) + H,O(1) + CO,(g) > The excess HCI(aq) is titrated by 4.60 mL of 0.125 M NaOH(aq). Calculate the mass percentage of CaCO,(s) in the sample. mass percentage:

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:

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

A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 626. mg of oxalic acid (H,C,04), 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 145.9 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits. MAR 3. ... MacBook 44 DI DD 000 000 F10 F9 F8

A titration analysis of a 24.0 mL aqueous HI solution was performed and the endpoint was reached upon the addition of 15.1 mL of 0.611 M aqueous calcium hydroxide solution. What is the concentration (in M) of the HI solution? HI(aq) + Ca(OH)2(aq) ——> CaI2(aq) + H2O(l)

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?