What mass of Ca(OH)2 is present in a sample if it is titrated to its equivalence point with 0.95L of 0.054 M HNO3? The balanced chemical equation is as follows: 2HNO3 + Ca(OH)2 --> Ca(NO3)2 + 2H2O The molar mass of Ca(OH)2 is 74.1g/mol
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- In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?If 1.000 ml. of a solution of KMn04 is equiva- lent to 0.1000 millimole of NaCHO2 (sodium formate) in the fol- lowing titration: 3CHO2- + 2MnO- + H2O -> 3CO2 + 2MnO2 + 5OH-, what is the value of the KMnO4 in terms of grams of CaO in the volumetric method for calcium in which that element is precipitated as CaC2 4 .H2O and the precipitate is filtered, dis- solved in dilute H2S04 , and the oxalate titrated with permanganate?
- The arsenic in a 1.22-g sample of a pesticide was converted toAsO43- by suitable chemical treatment. It was then titratedusing Ag+ to form Ag3AsO4 as a precipitate. (a) What is theoxidation state of As in AsO43-? (b) Name Ag3AsO4 by analogyto the corresponding compound containing phosphorusin place of arsenic. (c) If it took 25.0 mL of 0.102 M Ag+to reach the equivalence point in this titration, what is themass percentage of arsenic in the pesticide?3 L contaminated air 50 mL 0.0116 M in an air pollution analysisCarbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution.is precipitated as. Excess of base, next to phenol phthalate (f.f.) indicatorIt is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sampleCalculate its concentration in ppm. (Density of CO2Take it as 1.98 g / L. C = 12, O = 16 g / mol).1. 0.646 g of sample containing BaCl2.2H2O (244.26 g/mol) was dissolved and enoughpotassium chromate was added. After filtering, the precipitate was dissolved in acid andenough KI was added and titrated with thiosulfate. Since 48.7 mL of 0.137 M thiosulfateis used for this, what is the percentage of BaCl2.2H2O in the sample?K2Cr2O7 + 7H2SO4 + 6KI 4K2SO4 + Cr2(SO4)3 + 7H2O + 3I2
- (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/LA 1.200-g sample of a mixture of NaOH (FW 40.00 g/mol) and NayCO3 (FW 105.99 g/mol) with inert impurity is dissolved in 100 mL water and titrated with 0.150 M HCI.With phenolphthalein as the indicator, a 50.00 mL aliquot of the solution turns colorless after the addition of 30.00 mL of the acid. Methyl orange is then added, and 7.00 ml more of the acid are required for the color to change to pink. What is the percentage of NaOH in the sample?0.0585 g Na2C2O4 10 mL to adjust KMnO4 solution prepared in 0.1 M'pure water, 2 M H2SO4 added, heating process and 8.4 mL titrant as a result of titration it's spin out. Calculate the actual concentration of potassium permanganate accordingly
- If Sn3(PO4)2 solution is to be subjected to argentometric titration, a) Write the balanced titration reaction. (products are Ag3PO4(s),, other ions are spectator ions b) Write the stoichiometric relationship (fundamental eqn) between the titrant (AgNO3) and the titrand (Sn3(PO4)2. c) Is this a feasible titration technique? Why?If 1.000ml of a solution of KMnO4 is equivalent to 0.1000mmol of sodium formate (HCO2Na) in the following titration: 2HCO2-+ 2MnO4-+ H2O → 3CO2 + 2MnO2 + 5OH-, what is the value of the KMnO4 in terms of grams of CaO in the volumetric method for calcium in which that element is precipitated as CaC2O4•H2O, the precipitate filtered and dissolved in dilute H2SO4, and the oxalate titrated with permanganate?As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4Cl. A 5.095 g soil sample was dissolved to give 0.500 L of solution. A 150.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+ and NH4+ ions completely. B(C6H5)4-+K+⟶KB(C6H5)4(s) B(C6H5)4-+NH4+⟶NH4B(C6H5)4(s) The resulting precipitate amounted to 0.269 g. A new 300.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH4+ as NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.129 g of precipitate. Find the mass percentages of NH4Cl and…