SOLVE mathematically, then choose the correct answers: Calculate the pH of solution made by combining 100 ml of 0.28 M HC,H,O, and 50 ml of 0.36 M NAOH, Ka for HC,H,O, =1.8 x 10 a- 3 b- 3.68 c- 4.74 d- 5 c- 6 2- The pH in a saturated Mn(OH); solution is...at solubility product constant for Mn(OH); is 4.6x10". a- 9.0 b- 9.2 c- 9.3 d- 9.5 e- 9.7
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- I would really appreciate some help in confirming a value computed in a prelab problem to be used in a lab for analytical chemistry! We're working on redox reactions and are looking at the reaction: Fe2+ + K2Cr2O7 + H+ = Fe3+ + K+ + Cr3+ + H2O The final questions asks, "calculate the amount of unknown sample needed to achieve about a 25.00 mL titration volume of 0.01600 M K2Cr2O7 if the %Fe of the unknown is approximately 8%. Make sure to use the coefficients from the balanced reaction" I have found the balanced equation; however, I was hoping to be able to confirm my values! Thank you in advance!Chromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.A solution contains 0.010 0 M IO3- , 0.010 0 M I-, 1.00 x 10-4 M I3-, and pH 6.00 buffer. Consider the reactions 2IO3- + I- + 12H+ + 10e- --> I3- + 6H2O E° = 1.210 V I3- + 2e- --> 3I- E° = 0.535 V Calculate E° for the conditions given. 0.178 V 0.424 V 1.381 V 1.120 V
- A 0.2386-g sample contained only NaCI and KBr. It was dissolved in water and required 48.40 mL of 0.04837M AgN03 for complete titration of both halides (giving AgCI(s) and AgBr(s)). Calculate the weight percent of Br in the solid sample.0.0322 M EDTA solution is used as the titrant in the titration of a 50.00 mL solution that is 0.0129 M in Cu2+. The solution is held at pH = 10.00 by a buffer that is 0.050 in ammonia (NH3). At what volume (in mL) of EDTA added will the equivalence point be reached?A 0.3285 g sample containing chloride and inert material is titrated with 0.1012 M AgNO3, requiring 34.99 mL to reach the Ag,Cro. end point. Titration of a blank sample consumes 0.32 mL of the AgNO, titrant. Determine the % w/w chloride in the sample.
- A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 MNa2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer untilthe pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator.Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, onwhich the solution will turn red. Calculate for the molarity of the unknown.A solution contains 0.010 0 M IO3- , 0.010 0 M I-, 1.00 x 10-4 M I3-, and pH 6.00 buffer. Consider the reactions 2IO3- + I- + 12H+ + 10e- --> I3- + 6H2O E° = 1.210 V I3- + 2e- --> 3I- E° = 0.535 V Calculate E° and K for the reactionThe sulfur content of insoluble sulfides that do not readilydissolve in acid can be measured by oxidation with Br2to SO42.25Metal ions are then replaced with Hby an ion-exchange column,and sulfate is precipitated as BaSO4with a known excess ofBaCl2. The excess Ba2is then titrated with EDTA to determinehow much was present. (To make the indicator end point clearer,a small, known quantity of Zn2also is added. The EDTA titratesboth the Ba2and the Zn2.) Knowing the excess Ba2, we cancalculate how much sulfur was in the original material. To analyzethe mineral sphalerite (ZnS, FM 97.46), 5.89 mg of powderedsolid were suspended in a mixture of CCl4and H2O containing1.5 mmol Br2. After 1 h at 20 C and 2 h at 50 C, the powder dis-solved and the solvent and excess Br2were removed by heating.The residue was dissolved in 3 mL of water and passed throughan ion-exchange column to replace Zn2with H. Then 5.000 mLof 0.014 63 M BaCl2were added to precipitate all sulfate as BaSO4.After the addition of…
- A buffer solution is formed by adding 0.200 moles of solid potassium nitrite, KNO₂, to 500.0 ml of 0.500 M Nitrous acid, HNO₂ solution. You may assume that the change in volume is negligible upon addition of the solid. pKa of HNO2 is 3.40 Ka of HNO2 is 4.0E-4 m.w. of HNO2 is 47.01 g/mol pH of the buffer solution is 3.30, so now Calculate the pH of the buffer solution after the addition of 5.00 ml of 2.50 M Ba(OH)₂.Compare the solubility of nickel(II) carbonate in each of the following aqueous solutions: 0.10 M Ni(CH3COO)2 0.10 M (NH4)2CO3 0.10 M KNO3 0.10 M NH4CH3COO More soluble than in pure water. Similar solubility as in pure water. Less soluble than in pure water.Using basic conditions, MnO4- can be used as titrant for the analysis of Mn2+, with both the analyte and the titrant ending up as MnO2. In the analysis of a mineral sample for manganese, a 0.5165-g sample is dissolved, and the manganese is reduced to Mn2+. The solution is made basic and titrated with 0.03358 M KMnO4, requiring 34.88 mL to reach the endpoint. Calculate the %w/w Mn in the mineral sample. Answer: % Mn =