Fundamentals Of Analytical Chemistry
9th Edition
ISBN: 9781285640686
Author: Skoog
Publisher: Cengage
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A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate the molar analytical concentration of K3Fe(CN)6.
A 0.709 g sample of H2C2O4·2H2O is dissolved in water and titrated to a phenolphthalein endpoint with 27.98 mL of a sodium hydroxide solution. What is the molarity of the NaOH?
Gold is isolated from rocks by reaction with aqueouscyanide, CN-: 4 Au(s) + 8 NaCN(aq) + O2(g) + H2O(l)-------->4 Na[Au(CN)2](aq) + 4 NaOH(aq). (a) Which atoms fromwhich compounds are being oxidized, and which atomsfrom which compounds are being reduced? (b) The[Au(CN)2]- ion can be converted back to Au(0) by reactionwith Zn(s) powder. Write a balanced chemical equationfor this reaction. (c) How many liters of a 0.200 M sodiumcyanide solution would be needed to react with 40.0 kg ofrocks that contain 2.00% by mass of gold?
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- What volume of 0.200 M NaOH is necessary to neutralize the solution produced by dissolving 2.00 g of PCl3 is an excess of water? Note that when H3PO3 i5 titrated under these conditions, only one proton of the acid molecule reacts.arrow_forwardCalculate the molarity of AgNO3 in a solution prepared by dissolving 1.44 g AgNO3 in enough water to form 1.00 L solution.arrow_forwardPhosphate buffers are important in regulating the pH of intracellular fluids. If the concentration ratio of H2PO4/HPO42 in a sample of intracellular fluid is 1.1: 1, what is the pH of this sample of intracellular fluid? H2PO4(aq)HPO42(aq)+H+(aq)Ka=6.2108arrow_forward
- Exactly 750.0 mL of a solution that contained 480.4 ppm of Ba(NO3)2 were mixed with 200.0 mL of a solution that was 0.03090 M in Al2(SO4)3. (a) What mass of solid BaSO4 was formed? (b) What was the molar concentration of the unreacted reagent [Al2(SO4)3 or Ba(NO3)2]?arrow_forwardA student uses 7.500 grams of oxalic acid (H₂C₂O₄) to make 250.0 cm³ of solution in a volumetric flask. She then transfers 20.0 cm³ of the solution to a conical flask with a pipette. What is the concentration in mol·dm⁻³ of the oxalic in the conical flask?arrow_forward(a) Describe how to prepare 0.500 L of a 0.100 M aqueous solution of potassium hydrogen carbonate (KHCO3).(b) Describe how to dilute this solution to a final concentration of 0.0400 M KHCO3.arrow_forward
- b)4 A wastewater contains 7.2 mg L-1 phosphorus and is treated with 15 mg L1 aluminum in the form of an alum solution. Assume that phosphorus is precipitated out by Al3+(aq) + PO43 (aq) – AIPO4(s) and that any excess added aluminum forms Al(OH)3. Calculate the mass of inorganic sludge produced in one day in a plant treating 20000 m3 of wastewater.arrow_forward(b) An impure sample of (COOH)2.2H2O that had a mass of 1.00 g was dissolved in water and titrated with standard NaOH solution. The titration required 19.16 mL of 0.198 M NaOH solution. Calculate the percent (COOH)2.2H,O in the sample. Assume that the sample contains no acidic impurities. [molecular weight (COOH),.2H,O = 126 g/mol]arrow_forward(a) Which of the following compounds is/are soluble in water at room temperature?(i) Magnesium carbonate(ii) Strontium nitrate(iii) Potassium iodide(iv) Iron hydroxide(b) When an aqueous solution of sodium hydroxide is added to an aqueous solution ofiron(III) nitrate, a red/brown gelatinous solid is formed. Write a balanced molecularequation for the reaction that is taking place. Now rewrite your equation in net ionicform.arrow_forward
- 13.) Calculate the mass of solid MgSO̟•7H,O that must be added to precipitate out all of the PO,3- ions in the form of MgNH¸PO¸ •6H,O from 10.0 mL of a 2.0 M solution of PO,³ (aq)?arrow_forward(a) Predict the identity of the precipitate that forms when solutions of BaCl, and K,SO, are mixed. (b) Write the balanced chemical equation for the reaction.arrow_forwardQ1. A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate (a) the molar analytical concentration of K-Fe(CN)6- (b) the molar concentration of K+. (c) the molar concentration of Fe(CN) (d) the weight/volume percentage of K3Fe(CN)6. (e) the number of millimoles of K1 in 50.0 mL of this solution. (f) ppm Fe(CN)6¹arrow_forward
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