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)

Lead(II) nitrate and ammonium iodide react to form lead(II) iodide and ammonium nitrate according to the reaction Pb(NO3)₂(aq) + 2 NHI(aq) →→→ Pbl₂ (s) + 2NH4NO₂ (aq) · What volume of a 0.230 M NH4I solution is required to react with 289 mL of a 0.340 M Pb(NO3)2 solution? volume: 854.4 How many moles of Pbl2 are formed from this reaction? moles: 196.5 Incorrect mL mol Pbl₂

Calculate the number of milliliters of 0.587 M KOH required to precipitate all of the Mg²+ ions in 102 mL of 0.753 M MgCl₂ solution as Mg(OH)2. The equation for the reaction is: MgCl₂ (aq) + 2KOH(aq) → Mg(OH)2 (s) + 2KCl(aq) Volume = mL

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 13.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 11.9mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.

A 18.5 mL sample of Ba(OH)2 is titrated with HCl. If 37.5 mL of 0.921 M HCl is needed to reach the endpoint, what is the concentration (M) of the Ba(OH)2 solution?   Ba(OH)2(aq) + 2 HCl(aq) → BaCl2(aq) + 2 H2O(l)

A 0.124 M NaOH(aq) solution was used to titrate 20.00 mL of an acetic acid (CH3COOH) solution that has an unknown concentration. The equivalence point is reached after adding 15.34 mL of NaOH(aq). a) Write out the complete balanced equation for the reaction that occurs in this titration. b) How man moles of NaOH were added to the acetic acid solution? c) How many moles of acetic acid were in the original 20.00 mL solution? d) What was the concentration of acetic acid in the orignial 20.00 mL solution?

Calculate the number of milliliters of 0.650 M NaOH required to precipitate all of the Zn2+ ions in 119 mL of 0.478 M Zn(NO3)2 solution as Zn(OH)2. The equation for the reaction is:Zn(NO3)2(aq) + 2NaOH(aq) Zn(OH)2(s) + 2NaNO3(aq)

Calculate the molarity of an acetic acid solution if 26.0 mL of an HC2H3O2 solution is titrated with 24.8 mL of a 0.169 M KOH solution: HC₂H3O2 (aq) + KOH(aq) → H₂O(1)+ KC₂H3O2 (aq) Express your answer with the appropriate units.

A solution of permanganate is standardized by titration with oxalic acid, H₂C₂O4. To react completely with 1.000 × 10-³ mol of oxalic acid required 35.29 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is MnO4 (aq) + H₂C₂O4 (aq) → →Mn²+ (aq) + CO2 (9) Determine the concentration of the permanganate solution in molarity. Concentration = M

To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.3600M silver nitrate AgNO3 solution to a 24.00g sample of the fluid and collects the solid silver chloride AgCl product. When no more  AgCl is produced, he filters, washes and weighs it, and finds that 1.28g has been produced. The balanced chemical equation for the reaction is: Cl−(aq) + AgNO3(aq) -> AgCl(s) + NO−3(aq) What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Cl in the sample. Be sure your answer has the correct number of significant digits.