NAOH (ag) + HCI NaCl (ag) + H20 (1) (aq) -> 31.88 mL of 0.09951 M NaOH was used to titrate 7.00 mL of HCI to the endpoint. Calculate the mol of HCI that reacted and the molarity of the HCI solution. SHOW WORK. Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, molarity = M Enter where each reactant is placed at the beginning of the experiment (options are buret or flask): NaOH: HCl: Use the three blanks to enter the number, unit, and substance (in this order) that appears in the numerator of the stoichiometry conversion factor. Calculate the mol of HCl that reacted and enter the value only (decimal notation, including proper s.f.). mol Calculate the molarity of the original HCl solution and enter the value only (decimal notation, including proper s.f.). M

NAOH (ag) + HCI NaCl (ag) + H20 (1) (aq) -> 31.88 mL of 0.09951 M NaOH was used to titrate 7.00 mL of HCI to the endpoint. Calculate the mol of HCI that reacted and the molarity of the HCI solution. SHOW WORK. Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, molarity = M Enter where each reactant is placed at the beginning of the experiment (options are buret or flask): NaOH: HCl: Use the three blanks to enter the number, unit, and substance (in this order) that appears in the numerator of the stoichiometry conversion factor. Calculate the mol of HCl that reacted and enter the value only (decimal notation, including proper s.f.). mol Calculate the molarity of the original HCl solution and enter the value only (decimal notation, including proper s.f.). M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Given the following information: hydrocyanic acid HCN nitrous acid Ka = 4.0×10-10 HNO₂ K₂ = 4.5×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.370 M aqueous hydrocyanic acid and sodium nitrite are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium the ( reactants OR products) will be favored. (choose one answer) (3) The pH of the resulting solution will be ( greater than, equal to, OR less than 7). (choose one answer)
1.15 g of an unknown triprotic acid (H3A) is titrated with 2.50 M KOH. It takes 35.5 mL of KOH to reach the equivalence point of the titration. Calculate the molar mass of the unknown acid. H3A (aq) + 3 KOH (aq) → 3 H2O (l) + K3A (aq)
c. A JU student was asked to prepare a pH = 4.0 acid solution in which the molarity of H is 1.0 x 104 M. The only acid that is available is sulfuric acid, H2SO4. Assume that H2SO will completely dissociate according to Eq. 1. H2SO, (aq) So (aq) + 2H (aq) (1) First, the student transferred 1.500 mL pure H.SOa into a volumetric flask and made 200.0 mL solution (solution 1). The density of pure H2sO4 is 1.84 g/mL. Then he transferred exactly 10.00 mL solution 1 with a pipet into another volumetric flask and made 250.0 mL solution (solution 2). Please calculate the molarities of both solutions for him. If he can solve this problem correctly, it will prove to his supervisor he has necessary skills. WPXO 15 EFFEESEF MacBook Air
For the titration of 20.0 mL of 0.150 M acetic acid (CH₂COOH, K₂ = 1.8x105) with 0.150 M NaOH, what volume of NaOH is needed to reach the equivalence point? CH₂COOH(aq) + NaOH(aq) → NaCH3COO(aq) + H₂O(1)
Use the equation below to calculate the following: 2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l) (a) the grams of Na2SO4 that can be obtained from 25 mL of 0.050 M NaOH (b) the volume of 0.250 M H2SO4 needed to react with 25.5 mL of 0.750 M NaOH (c) the molarity (M) of the NaOH solution when 48.20 mL react with 35.72 mL of 0.125 M H2SO4
Calculate the concentration of HC6H₁06 in an aqueous solution of 4.81x10-2 M ascorbic acid, H₂C6H6O6 (aq). [HC6H606] = M.
One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9
Calculate the % relative error in hydronium ion concentration by using concentrations instead of activities in calculating the pH of the following buffer solutions using the thermodynamic constants listed below. Acid Formula K₂ Acetic acid CH, COOH 1.75 x 10-5 Ammonium ion NH₂+ 5.70 x 10-10 Chloroacetic acid CICH, COOH 1.36 x 10-³ b 0.0340 M NH3 and 0.120 M NH, CI Relative error = C 0.0210 M CICH₂ COOH and 0.0570 M CICH₂ COONa (αCICH, COO = 0.35) Relative error =
Annette and Marilyn are given four reactions involving acids and bases. A dark arrow facing left (B -->) means the reaction favours the reactants. A dark arrow facing right ( Products L(aq) + HM(aq) HM(aq) +R (aq) HN(aq) + M¯(aq) HL(aq) + N(aq) Based on this information, the girls determine the correct list of BASES from strongest to weakest as: a. R¯(aq) L-(aq) N-(aq) M-(aq) b. N-(aq) M-(aq) R-(aq) L¯(aq) c. L'(aq) R-(aq) M-(aq) N-(aq) d. M (aq) N-(aq) R (aq) L (aq)
Consider the titration of 25.0 mL of 0.125 M acetic acid (CH, COOH, pKa = 4.75) with 0.102 M NaOH. CH, COОН(aq)+NaOH(aq) — СH, СОО" (аq) + H,О1) + Na*(aq) Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.102 M NaOH is added. pH = Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.
Determine the pH at the equivalence (stoichiometric) point in the titration of 48.38 mL of 0.171 M HCN (aq) with 0.135 M NaOH(aq). The Ka of HCN is 4.9 * 10^-10.
Calculate the concentration of HNO3 (aq). Estimate the Kb for C2H5NH2 (aq) using the titration curve.