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- To analyze an aspirin sample, 0.3470 g of crushed tablets are weighed and treated with 50.00 mL 0.1155 M sodium hydroxide, boiling for 10 minutes. Under these conditions the acid acetylsalicylic (MW, 180) reacts according to: CH3COO-C6H4-COOH + 2 OH- → OH-C6H4-COO- + CH3COO- The excess NaOH is then titrated with 11.5 mL of 0.2100 M HCl. What is the purity of said show ?.A fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH)(COOH)(CH2COOH)2, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.(a) If the molar solubility of Cd3(AsO4)2 at 25 oC is 1.15e-07 mol/L, what is the Ksp at this temperature?Ksp = __________(b) It is found that 8.90e-06 g of Y2(CO3)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Y2(CO3)3.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3? solubility = ________mol/L
- NH3 is a weak base. It ionizes in water to produce NH4+ and OH-. Its Kb = 1.8 10-5 and Kw = 1 10-14 at 25oC. Please complete following tasks for a solution of 0.0500 M NH3 (aq) at 25oC. (A) concentration of NH4+A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate (a) the molar analytical concentration and Normality of K3Fe(CN)6. (b) the molar concentration of K+. (c) the molar concentration of Fe(CN)63-. (d) the weight/volume percentage of K3Fe(CN)6.Calculate the solubility of CaSO4 (in g·L-1) in the following media. The solubility product of CaSO4 is 4.9×10-5. Assume ideal behavi (a) water I-7.6 (b) a 7.8x10-5 M SrSO4 solution g•L-1
- A chemist receive different mixtures for analysis with the statement that it contain NaOH, NaHCO3 , Na2CO3 or compatible mixtures of these substances together with the inert material. From the data given, identify the respective materials and calculate the percentage of each component. 1.000g samples and 0.2500 N HCl were used in all cases. Sample 1 With phenolphthalein as the indicator, 24.32 ml of HCl was used. A duplicate sample required 48.64 ml HCl using methyl orange as the indicator. Sample 2. With phenolphthalein as the indicator it uses 28.2 ml of HCl to make it colorless and added with methyl orange indicator and uses 11.3 ml of HCl to reach the end point.given the Ksp of CaSO4 is 4.93 x10^-5 mol^2 L^-2, what is its solubilityWhat weight of potassium hydrogen phthalate will require 30. mL of a 0.30M NaOH solution to reach the equivalence point? KHP MM 204.22 g/mol .CO;K' .CO;K' NaOH + H2O + *CO,H COƠ,Na'
- Five drops of dichlorofluorescein have been added to a solution containing 0.800 g sample which required 25.30 mL of 0.100 M AgNO3. (c) Calculate the weight percent NaCl in the original sample.Lead(II) carbonate, PbCO3, is one of the components of thepassivating layer that forms inside lead pipes. (a) If the Kspfor PbCO3 is 7.4 x 10 - 14 what is the molarity of Pb2+ ina saturated solution of lead(II) carbonate? (b) What is theconcentration in ppb of Pb2+ ions in a saturated solution?(c) Will the solubility of PbCO3 increase or decrease as thepH is lowered? (d) The EPA threshold for acceptable levelsof lead ions in water is 15 ppb. Does a saturated solution oflead(II) carbonate produce a solution that exceeds the EPAlimit?20 puan a) Calculate the concentration of a solution containing 0.0056g Cr(II) in 12 g water as ppm.