1. 0.10 mol weak acid HCNO is dissolved in 1.00L H2O. What is the activity coefficient of CNO- and HCNO? 2. A 100mL sample of a solution contains 68.5 ng As. What is the concentration of As in ppb if the density of the sample is 1.20g/mL?
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1. 0.10 mol weak acid HCNO is dissolved in 1.00L H2O. What is the activity coefficient of CNO- and HCNO?
2. A 100mL sample of a solution contains 68.5 ng As. What is the concentration of As in ppb if the density of the sample is 1.20g/mL?
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- Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20 × 10–5, what is the Ksp value for LQ?A mixture of NaBr, Nal and NaNO3 weighs 0.6500 g. With AgNO3, a precipitate of the two halides is obtained and is found to weigh 0.9390 g. When heated in a current of C2, the precipitate is converted entirely to AgCi weighing 0.6566 g. What is the %NaNO3 in the original sample?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 solution contains dissolved PbCl2. There are 0.02575 moles Pb2+ and 0.0515 moles Cl-. a) What is the ionic strength of the PbCl2? b) What is the math expression for the thermodynamic solubility product of PbCl2, in which the ion activities are used in place of molar concentrations? c) What is the math expression relating the ion activity to the molar concentration? d) What is the math expression for the activity coefficient of an ion according to Extended Debye-Hückel approach?The phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN for titration to the FeSCN2+ end point. Calculate the percentage of phosphate in the detergent.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.
- If you want to dissolve 0.225 grams of AgBr, what volume of 0.0138M Na2S2O3 in mililiters, should be usedA 0.64 g sample containing KCl ( mw = 74.6 ) is dissolved in 50mL of water and titrated to the Ag2CrO4 end point, requiring 26.2 mL of 0.15 M AgNO3 .The %w/w KCl in the sample is ?The 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…
- Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2+(aq) and 0.0260 M Ag+(aq). What will be the concentration of Ca2+(aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, ?sp, can be found in the chempendix. [Ca2+]= M What percentage of the Ca2+(aq) can be precipitated from the Ag+(aq) by selective precipitation? percentage:(a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/L0.2219 g of pure iron wire was dissolved in acid nd iron reduced to+2 state. Then the solution required 34 65ml of cerium(4) in a titration . Calculate molar concentration of ce4+???