calculate the following: Vos = 20.20 ml (Cro.') = 0.1350 M (Ag') = 0.202 M Kıp = 1.17x 101 M a) Balanced Reaction b) Equivalence point volume (Ver) c) pAg @ 18.00 ml
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- At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6. (a) Write an expression for the solubility product of PbCrO4.(b) Calculate the solubility of PbCrO4.(c) On adding concentrated aqueous lead(II) nitrate dropwise to 0.010 moldm-3 potassium chromate (VI), what is the concentration of lead(II) ions when the first trace of precipitate appears?The solubility product constant of barium fluoride in water at 25o C is Ksp = 1.3 x 10-6. Calculate the solubility of this compound in 1.00 M Ba(NO3)2 (aq) at 25o If 15 mL of 0.024 M lead (II) nitrate is mixed with 30 mL of 0.030 M potassium chromate, will a precipitate form? (Ksp = 2.0 x 10-16 for PbCrO4) Calculate the ionic strength of the following solutions: 25 M Cr(NO3)3 05 M Al(ClO4) Using simple Debye-Huckel equation, estimate the following activity coefficients: SO42- at µ = 0.025 Fe(CN)63- at µ = 0.005 The solubility product constant of cuprous chloride in water at 25o C is Ksp = 1.0 x 10-6. Calculate the solubility of this compound in 0.020 M KCl(aq) at 25oA solution contains 2.0 x10-4 M Ag+(aq) and1.5 x 10-3 M Pb2 + (aq). If NaI is added , wi l l AgI(Ksp = 8.3 x10-17)or PbI2 (Ksp = 7.9x 10-9) precipitatefirst? Specify the concentration of I-(aq) needed to beginprecipitation.
- A student is calculating the concentration of her standard solutions in order to create the calibration curve (standard curve). Calculate the equilibrium isothiocyanatoiron(III) ion concentration, [FENCS²*]eg; for a solution created by leq combining 2.00 mL of 0.194 M Fe³* (aq) with 200PL of 0.00210 M SCN¯ (aq). Give your answer to three decimal places. Also give your answer in millimolar (mM) (because you won't be able to enter an answer in scientific notation here). You may assume that the volumes of these dilute, aqueous solutions are additive.Please use the values in the resources listed below instead of the textbook values. Perform the following calculations involving concentrations of iodate ions. (a) The iodate ion concentration of a saturated solution of Ce(IO3)4 was found to be 7.35X10 mol/L. Find the Ksp: 4.0 (b) Find the concentration (in M) of iodate ions in a saturated solution of Ra(IO3)2. (Ksp = 1.16X 10-9) 4.0) M2. In the titration of 50 ml. of 0.05 M of AGNO; solution with 0.05 M KSCN solution, calculate the molar concentration of Ag* in the conical flask solution after the following additions of titrant KSCN solution (Kp - [Ag*|[SCN]- 1.0 X 10-12): (a) 25 mlL (b) at equivalent point (c) 55 mL
- Moles SCN- used in titration (mol)Moles of Agt in 20.0 mL titrated (mol) [Ag*lequil (M)X= [Ag*Jinit - [Ag*lequil = Change (M) solve for flask d e and fA student is calculating the concentration of her standard solutions in order to create the calibration curve (standard curve). Calculate the equilibrium isothiocyanatoiron(III) ion concentration, [FeNCS²+]eq, for a solution created by combining 2.00 mL of 0.183 M Fe3+ (aq) with 225μL of 0.00199 MSCN- (aq). Give your answer to three decimal places. Also give your answer in millimolar (mM) (because you won't be able to enter an answer in scientific notation here). You may assume that the volumes of these dilute, aqueous solutions are additive.Do the argentometric titration according to given data and fill in the blanks. Ag+ (aq) + Cl- (aq) → AgCl (s) (White) NaCl » Na* + Cl- SET 2 Measured Weight of NaCl, (gr) 2.5 g Measured Weight of Cl- , (g) Volume of Stock Solution, (mL) 200 mL Amount of Sample taken from the stock solution, (mL) 9mL Normality of AgNO3, (N) 0.1 N Initial burette reading, (mL) O mL Final burette reading, (ml) 6.85 mL Volume of AgNO; Consumed, (mL) 6.85 mL Amount of AGNO3 Consumed, (mg) Calculated Weight of NaCI in stock Solution, (g) Calculated Weight of CI- in stock Solution, (g) Error in Calculating Amount of CI-(%)
- Select the correct mass balance equation for a saturated solution of CaCl₂ assuming that the ionic species are Ca²+, Cl-, CaCl and CaOH+. (A) (B) (C) (D) O O (A) (B) (C) (D) [CH]+[CaCl] = 2[Ca²+] + 2[CaCl*] + 2[CaOH*] [CI] + [CaCl] = 2 [Ca²+] + [CaCl*] + [CaOH*] [CI]+[CaCl] = [Ca²+] + [CaCl+] + [CaOH+] [CI] = [Ca²+] + [CaOH+]2a Suppose the Gapon constant K =([Ca ] X/([Cd ]X.) is 25. Also suppose that your soil has equilibrated with a large mass of contaminated water with a [Ca ] of 0.1 millimoles per liter and a [Cd ] of 0.025 millimoles per liter. What is the X/X. in the soil? 2b. Suppose the CEC of the soil is 0.3 milliequvalents per kilogram and assume that the only two cations attached to the soil particles are Ca and Cd What is the total amount of Cd attached to a kilogram of soil. 2c. Suppose that an area of soil 300 meters long, 200 meters wide and 2 meters deep with a density of 1800 kilograms per cubic meter has been contaminated with this water. What is the total mass of Cd in this soil?Calculate the molar solubility of LizPO4 (Ksp =2.37 x 10-") in a ID 0.0379 M lithium nitrate (LINO3) solution.