Calculate the concentration of an HCI solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)₂ to reach the titration endpoint. Mg(OH)₂ + 2 HCI 2 H₂O + MgCl₂ There is enough information to calculate the moles of base but not the moles of acid. mol ( L)(- mol Mg(OH)3 mol HCI ( mol Mg(OH)3)(- mol HCI mol Mg(OH)2 mol HCI L a. 0.1000 h. CaCO3(s) 0. H₂PO4¹ v. H₂CO3 bb. 3.300 x 10-² hh. 2.16 x 10-6 b. 0.1320 i. OH-¹ p. CO3-² W. PO43 C. HX j. H30+1 q. HCO3-1 x. HC₂H302 dd. 2 cc. 3 ii. 1.60 x 10-5 = d. Al+3 K. SO4² r. H₂S jj. 0.2000 L e. CO₂ y. C₂H30₂-1 ee. 1 I. Mg+2 S. HS-1 -) = M HCI f. CaF2(aq) m. Cl-1 t. S-2 z. 1 x 10-14 ff. 0.099536 kk. 6.600 x 10-3 -) = g. HF (aq) n. HPO4² u. H₂O(liq) aa. 1.32 x 10-² gg. 3.95 x 10-3

consider the titration of 50.0 mL of 0.10 M acetic acid with NaOH. drag and drop each amount of NaOH added (to the acetic acid) Into the appropriate resulting pH. In other words, determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solutions be acidic, basic, or neutral? Consider the stration of 50.0 ml of 0.10 M acetic acid (HC₂H₂O₂. K, -18 x 10) with NaOH. Drag and drop each amount of NaOH added to the acetic acid) into the appropriate resulting pH. In other words determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solution be acidic, basic, or neutra? Acidic Neutral Basic Drag and drop your selection from the following list to complete the answer 25.0 mL (total) of 0.10 M NaOH has been added (the halfway point) 50.0 mL. (total) of 0.10 M NaOH has been added (the equivalence point) 10.0 mL (total) of 0.10 M NaOH has been added 60.0 mL (total) of 0.10 M NaOll has been added No NaOH has been…

A 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of the acid), was dissolved in water and titrated with 0.150 M barium hydroxide solution. The titration required 13.9 mL of the base to reach the equivalence point. What is the molar mass of the acid? 227 g/mol 82.5 g/mol 371 g/mol 124 g/mol 186 g/mol

2) Part way through a titration, 2.0 x 10¹ mL of 0.10 mol/L sodium hydroxide has been added to 3.0 x 10¹ mL of 0.10 mol/L hydrochloric acid. a) what is the pH of the solution? b) What is the pOH of the solution? c) what is the concentration of H+ ions in the solution?

Consider the following reactions: Reaction 1: HCIO, + KOH → KC1O, + H;O Reaction 2: HC;H;O2 + KOH → KC;H;O2+ H;O In both reactions, 15.00 mL of 0.8116 M acid is titrated with 0.4217 M KOH. A volume of 28.87 mL of KOH is required to reach the equivalence point in both reactions. a) What is the pH of the HC1O, solution before the titration has started? (No KOH has been added.) b) What is the initial pH of HC;H;O2 solution before the titration has started? K= 6.46 x 10-5 (Ok to use x is small.) c) What is the pH of Reaction 1 at the equivalence point? d) What is the pH of Reaction 2 at the equivalence point? e) What is the pH of Reaction 1 after 32.00 mL of KOH has been added? f) What is the pH of Reaction 2 after 18.00 mL of KOH has been added?

Consider the following information to answer the questions below. A volume of 10.00 mL of 0.100 M acetic acid (HC2H3O2) is titrated with 0.107 M sodium hydroxide solution. Given the chemical equation below. Calculate the volume (in milliliters) of NaOH needed to reach the equivalence point of the titration. HC2H3O2(aq) + NaOH(aq) -> H2O (l) + NaC2H3O2(aq)

Part 3 Prepare a data table for the titration of NaOH with diluted vinegar. Include enough data columns for at least 3 titrations. PRELAB QUESTIONS 1. Calculate the molar mass of Potassium acid phthalate, KHC8H404 (KHP). You will use this number to do the calculations for part 1 once you do the titration. 2. Calculate the molar mass of acetic acid, HC₂H3O2. You will use this number to do the calculations for part 3 once you do the titration. 3. Solve the following problem: If it takes 35.04 mL of a 0.2455 M NaOH solution to neutralize 25.00 mL of an unknown HCl solution, what is the molarity of the HCl solution? Use the roadmap given under part 2 to calculate this problem. MA Chemistry 60 lab Page 110 3

50.00 mL of a buffer solution contains 0.280 M HClO and 0.450 M NaClO.  If 25.00 mL of water is added to the buffer, what are the new concentrations of HClO and NaClO?

-2 What volume in milliliters of 9.850 x 10 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 14.0 mL sample of 0.144 M phosphoric acid? Express your answer using three significant figures.

In a titration, if 12.00 mL of vinegar requires 19.85 mL of 0.4500 M NaOH to reach the equivalence point. What is the molarity of the vinegar solution? Hint: Vinegar contains acetic acid (HC2H3O2).