Based on the reported saturation points (in m/v %), which of the following compounds is the most soluble? aluminum sulphate (36,4%) barium acetate (75,0%) calcium bicarbonate (16,6%) lead(ii) nitrate (54,3%) lithium hydroxide (12,8%)
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- (1) Careless Carlie weighed her KHP sample, but forgot to bring her report sheet along, so she recorded the mass of KHP on a paper towel. During her titration, which required 18.46 mL of base, she spilled some base on her hands. She remembered to wash her hands, but forgot about the data on the towel, and used it to dry her hands. When she went to calculate the molarity of the base, Carlie discovered that she didn’t have the mass of her KHP. Her kindhearted instructor told Carlie that her base was 0.2987 M. Calculate the mass of Carlie’s KHP sample. Show calculations (2) What mass of solid NaOH would be needed to make 645 mL of Carlie’s NaOH solution? Show calculations.A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.1. A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer? 2. Data in the table below were collected at 25°C for the following reaction:2 I–(aq) + S2O82–(aq) I2 (aq) + 2 SO42-(aq) a) Determine the rate law for the reaction. b) Calculate the rate constant, giving the correct units for k.
- A sample containing chlorophenol, C6H4ClOH, was analysed by gravimetric analysis. A 0.783-g of this sample goes through a chemical process allowing the chlorine in the chlorophenol to precipitate as silver chloride, weighing 0.271 g. Calculate the % (wt/wt) of the chlorophenol in the sample, assuming that chlorophenol is the only source of chlorine in the sample. Provide your answer to two decimal places and without units. Avoid using scientific notation.Can you please help me with a, b, c and d A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 a) Calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer. b) Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer. c) Calculate the pH of the buffer solution. d) What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer?5) The solubility of BaCO3 is 24 mg/L at room temperature. a. What is the molar solubility and the Ksp of barium carbonate? b. The carbonate ion can react with water as follows: CO3² (aq) + H₂O (1) HCO3 (aq) + OH- (aq) Kb = 2.1 x 10-4 Write the reaction out from part a, add the two reactions together, and calculate the new K of the combined reaction. C. Using your K from part b, find the solubility of BaCO3 when the reaction in part b is also considered. Did the solubility increase or decrease from part a? Explain using Le Chatelier's Principle.
- A mixture containing KCl and NaBr was analyzed by Mohr's method. A mass of 0.31011 g of the mixture was dissolved in 50 mL of water, the Na2CrO4 indicator was added, and it was titrated with a 0.11011 mol/L AgNO3 solution. The endpoint was 36.011 mL. What are the % m/m concentrations of KCl and NaBr in the mixture?When a Vitamin C (ascorbic acid; MM = 176.12 g mol-1) tablet is crushed, dissolved and titrated with 0.0340 M KIO3(aq) to a purple/blue endpoint (given by a starch indicator), the volume of KIO3 used is 29.80 mL. If 60 mg of ascorbic acid is the recommended dietary allowance (i.e., 100% of the RDA), then what is the % RDA for the Vitamin C in the tablet? KIO3(aq) + 5 KI + 6 H+ → 3 I2(aq) + 3 H2O I2 (aq) + ascorbic acid → 2 I- + dehydroascorbic acidConsider a saturated solution of benzoic acid in water. Dichloromethane (a non-polar solvent) was added to the aqueous mixture, and the resulting mixture was mixed. After a while, a formation of two layers was observed. Given the structure of benzoic acid. Which of the following statements is TRUE? H ... H. HO H. benzoic acid A Benzoic acid will remain in the aqueous layer. B Benzoic acid will react to form sodium benzoate. Benzoic acid will be more soluble in the dichloromethane layer. D Benzoic acid will crystallize in the aqueous layer.
- As part of this experiment you will need to determine the concentrations of Fe* and SCN ions present in test tubes 1-9. These values can be calculated using the volumes and concentrations provided in Tables 1 and 2 of the Equilibrium Lab - Procedure and the dilution equation (M,V1 = M2V2). Note: the solutions provided in the lab, and therefore the tables in the lab document, are the compounds used to prepare the solution. You must determine the concentration of the ions based on how these compounds díssociate in solution Complete the following table by filling the the calculated initial concentrations of each substance. Be sure to: Pay attention to significant figures • Round appropriately Use decimal notation (not scientific) Do not include units Test Initial [Fe3*] (M) Initial [SCN'] (M) Tube 1 3 4. 6. 7 8. 2.Calculate the percent by mass of oxygen in each of the following compounds: (a) Fe2O3 (b) Al2O3 A commercial mouthwash contains 4.5 g of ethanol and 0.022g antiseptic in each 30.-mL portion. Calculate the w/v percent concentration of each component. How many mL of ethanol are contained in a 30.-mL portion of mouthwash that has 8.5%(v/v) of ethanol? A cough medicine contains 0.22% (w/v) dextromethorphan, a cough suppressant , and 2.2% (w/v) guaifenesin, an expectorant. How many mg of each drug would you obtain from 3.0 tsp of cough syrup? (1 tsp = 5 ml)The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?
