A 0.434 g sample of a monoprotic acid is dissolved in water and titrated with 0.170 M KOH. What is the molar mass of the acid if 18.5 mL of the KOH solution is required to neutralize the sample? molar mass: g/mol
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- (f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)9. Solid sodium carbonate, Na,CO, is used to determine the concentration of a HBr(aq) by titration. What is the role of sodium carbonate in this titration? (A) Catalyst (B) IndicatorA8 (C) Primary standard (D)Proton donor euld bne el hotsolon (A) nielerd auld lom onolbni Vegnto nouloe s lo ophar Hq es Short Answer 1. Consider the following equilibrium for the chemical indicator phenol red, HInd, at pH = 7.3. 0.00 H,0 = H,O* + Ind red HInd + Yellow If 10.0 mL of 0.10 mol/L NAOH(aq) is added, how will the concentration of H,O* (aq) be affected, and what is the color of the resulting solution?To an aqueous solution containing 1.6000 g sample consisting of a mixture of CaBr2•H2O and inert matter, 52.00 mL of 0.200 M AgNO3 is added. The excess Ag+ requires 4.0 mL of 0.1000 M KSCN for the precipitation of AgSCN. What is the percentages of CaBr2 •H2O and of inert matter in the sample? Please provide a complete solution.
- 7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq) Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)True.00 mL of a nitric acid solution of unknown concentration is pipetted into a 125-mL Erlenmeyer ask and 2 drops of phenolphthalein are added. A 0.150M sodium hydroxide solution (the titrant) is bocd to titrate the nitric acid solution (the analyte), If 12.75 mL of the titrant is dispensed from a et in causing a color change of the phenolphthalein, what is the molar concentration of the nitric Sin acid solutionWhat minimum volume of 0.09621 M AgNO3 willbe needed to assure an excess of silver ion in the titration of: (a) an impure NaCl sample that weighs 0.2513 g?(b) a 0.3462-g sample that is 74.52% (w/w) ZnCl2?(c) 25.00 mL of 0.01907 M AlCl3?
- A buffer solution contains 0.387 M NaH,PO4 and 0.212 M K2HPO4. Determine the pH change when 0.061 mol HCIO, is added to 1.00 L of the buffer. pH change =| A buffer solution contains 0.229 M CGH;NH3CI and 0.381 M C,H3NH2 (aniline). Determine the pH change when 0.077 mol HCl is added to 1.00 L of the buffer. pH after addition – pH before addition = pH change =| A buffer solution is 0.301 M in HCN and 0.274 M in KCN . If K, for HCN is 4.0×10-10 , what is the pH of this buffer solution?A 250 ml solution is prepared with 1.5 g KCI salt and a 50 ml sample is taken from it. Over 40 ml 0,1100 N AGNO3 is being added. After AgCl is filtered off, it is titrated with KSCN with Fe (III) indicator. Since 5 ml of 0,1N KSCN is spent in the titration, can we find the amount of KCI and the percentage of KCI purity? (K. 39 g/ mol, CI: 35.5 g/mol)Tungsten trioxide (Wo,) has a rich yellow color and is often used as a pigment in ceramics and paints. To test a ceramic vase for its WO, content, a 10.11 g sample of the vase was ground and reduced with Pb(Hg) to convert any WO, to W+. The resulting w* was transferred to 500.0 mL. of 1.00 M HCI. A 100.00 ml. aliquot of the HCl solution required 13.18 mL of 0.08251 M I 1.00M potassium permanganate (KMNO,) to reach the purple endpoint. A blank required 0.15 ml.. Balance the redox reaction. redox reaction: Mno; + w* Mn* + wo?* Determine the percent Wo, in the ceramic sample. percent WO,:
- A buffer solution is prepared from a generic weak acid "HG" and the salt KG. The K, for HG is 3.7 x 106. What (net) chemical reaction will occur when HNO, is added to the busfer solution? O No reaction will occur. The buffer prevents reaction. O KG + HG + HNO, HKG+ + HNO,G- G-+ H3O' --> HG + H2O O HG + NO, -> HNO3 + G O HG + H3O --> H2G" + H2O1. 0.646 g of sample containing BaCl2.2H2O (244.26 g/mol) was dissolved and enoughpotassium chromate was added. After filtering, the precipitate was dissolved in acid andenough KI was added and titrated with thiosulfate. Since 48.7 mL of 0.137 M thiosulfateis used for this, what is the percentage of BaCl2.2H2O in the sample?K2Cr2O7 + 7H2SO4 + 6KI 4K2SO4 + Cr2(SO4)3 + 7H2O + 3I2When 38.0 mL of 0.1250 M H,SO, is added to 100. mL of a solution of PbI, a precipitate of PbSo, forms. The PbSO, is then filtered from the solution, dried, and weighed. If the recovered PbSO, is found to have a mass of 0.0471 g, what 4 was the concentration of iodide ions in the original solution? Select one: -4 a. 3.10 x 10 -3 b. 1.55 x 10 M C. 6.20 x 103 M -3 d. 3.11 x 10 M -4 e. 1.55 x 10 Previou