A 100.0 mL sample of 0.18 M HCIO, (Strong acid) is titrated with 0.27 M LIOH. Determine the pft of the solution after the addition of 30.0 mL of LIOH, a. 0.86 Ob. 1.21 Oc. 2.00 O d. 1.12
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- Use Table 17.1 to find Kffor AuCl4- (aq) at 25°C.A 0.0712-g sample of a purified organic acid was dissolved in an alcohol-water mixture and titrated with coulometrically generated hydroxide ions. With a current of 0.0392 A, 241 s was required to reach aphenolphthalein end point. Calculate the equivalent mass of the acid.A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the Ksp of magnesium hydroxide?
- 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.When 38.0 mL of 0.1250 M H,SO̟ 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 was the concentration of iodide ions in the original solution Select one: а. 1.55 х 10 M -3 b. 1.55 x 10 M -3 с. 6.20 х 10 -3 d. 3.11 x 10 M -4 e. 3.10 x 10 M ΣΣA saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the molar solubility of magnesium hydroxide?
- 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.The concentration of CO in air is determined by passing a known volume of air through a tube that contains I2O5, forming CO2and I2. The I2 is removed from the tube by distilling it into a solution that contains an excess of KI, producing I3-. The I3-is titrated with a standard solution of Na2S2O3. In a typical analysis a 4.79-L sample of air is sampled as described here, requiring 7.17 mL of 0.00329 M Na2S2O3 to reach the end point. If the air has a density of 1.23 × 10–3 g/mL, determine the parts per million CO in the airTungsten 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 50.00 mL of 0.100 M Fe(II) is to be analyzed by redox titration with suitable reagents For the redox titration of 50.00 mL of 0.100 M Fe(II) with 0.100 M Ce(IV) in1 M H2SO4, (i) What is the reaction involved? (ii) Explain how the potential at the equivalence point can be determined.Calculate the potential at the equivalence point as measured by a platinumindicator electrode against a standard hydrogen electrode.A student wanted to determine the amount of NaOCI in a commercial bleaching solution. He diluted 2 g of bleach in a 100 ml volumetric flask. A 50 ml sample of the diluted bleach was mixed with excess acidified potassium iodide KI and a few drops of an indicator. The resulting solution was titrated with Na-S.O, solution. The titration required 17 mL of 0.05M Na,S,O, solution. The series of reactions that take place during this experiment: 21+OCI+ 2H1₂ + Cl + H₂O 1₂+28,0,³ →21+S,0,² a) Calculate the number of moles of OCI- in 50 mL diluted bleach and in 100 mL.Consider the titration 35.0mL of 0.250M methylamine CH NH2 and 0.200 M HNO3. K. = 5.9 x 104 a. Determine the pH at the midpoint b.Determine the pH when 25.0 mL of titrant was added.