If 25.00 mL of 0.100 M AGNO3 is mixed with 25.00 mL of 0.300 M NaCN, find (Ag*], [Ag(CN)2], and [CN']. Kf, Ag(CN), = 7.08 x 1019 %3D L00A A N. concontratic
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- Calculate the concentration of cobalt(III) ions in a solution formed by mixing 200 mL of 0.200 M Co(NO3)3 with 250 mL of 5.00 M NH3 solution given Kf of [Co(NH3)6]3+ is 4.5×1033. [Co3+] = ___MWhat volume of 0.380 M KMnO4 would be required to titrate 0.33 g of K2[Cu(C2O4)2]⋅2H2O?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 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.(e) the number of millimoles of K+ in 50.0 mL of this solution.(f) ppm Fe(CN)63- .(g) pK for the solution.(h) pFe(CN)6 for the solution.
- A 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 accordinglyA sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 84.3-mL sample of this solution was withdrawn and titrated with 0.0948 M HBr. It required 64.6 mL of the acid solution for neutralization.(a) What was the molarity of the Ca(OH)2 solution? M(b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution? g/100mL
- In order to adjust the permanganate solution, the necessary experimental procedures were performed by taking 0.0585 g Na2C2O4 and the titrant consumption was 8.4 mL. Calculate the KMnO4 concentration accordingly (Na: 23, C: 12, O: 16 g / mol)The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3il? How many milliliters of concentrated sulfuric acid, 94.0% (w/w), specific gravity of 1.831 are required to prepare 1 liter of a 0.100 M solution? The solubility-product constant for Ce(IO3)3 is 3.2x1010. What is the Ce3+ concentration in a solution prepared by mixing 50.0 ml of 0.0250 M Ce3.. with 50.00 ml of water?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.
- A 1.7483-g sample containing Al(NO3)3, AlCl3, and inert material was dissolved in acid and divided into two equal portions. One portion was treated with 5.00 mmol of AgNO3. The excess Ag+ required 28.89 mL of 0.l002 M KSCN for titration. The other portion required 26.02 mL of 0.1193 M NaOH for titration:Al3+ + 3 OH- → Al(OH)3(s)Calculate the percentage composition of Al(NO3)3 and AlCl3 in the sample.A student weights out 1.118g of impure KHP, dissolves the sample in deionized water and titrate it with 0.1001 M NaOH solution. If the titration requires 27.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?What weight of sample in gram containing 8.00 % Fe3O4 (MW= 231.53 g/mole) must be taken to obtain a precipitate of Fe (OH)3 (MW= 106.867 g/mol) that, when ignited to Fe2O3 (MW = 159.69 g/mole), weighs 150.0 mg