The overall formation constant for Hgl is 1.0 x 10". What is the concentration of Hg in 500.0 ml. of a solution that was originally 0.10 M Hg" and 0.78 MI? The reaction is: Hg (ag) + 41 (ag)Hgl, (ag) 4.7x10-31 6.9 x10-31 1.8x10 30 2.6x1031 4.8x10-30
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- The overall formation constant for HgI42- is 1.0x1030. That is, 1.0x1030 = [HgI42-] / [Hg2+] [I-]4 What is the concentration of Hg2+ in 400.0 mL of a solution that was originally 0.016 M Hg2+ and 0.72 M I-? The reaction is Hg2+ (aq) + 4I- (aq) <----> HgI42- (aq) [Hg2+] = ____________ MNeutralization Titration In the standardization of HCI solution using 10.00 ml of 0.02 Na,co, according to the equation M of Na,CO, 2 HCI 2NaCl + H₂O+CO, 15.0 ml of HCI is required to reach the end point using Bromocresol green indicator the molarity of HCI (mol/L) would be al 0.032 b) 0.027 20.013 d) 0.008 e) 0.064Calculate the molar solubility of Ag2S in a solution maintained at pH 11.00 and where the concentration of free ammonia is 0.100 M. Ag2S: pKsp = 48.70H2S: Ka1 = 1.0 x 10-7 ; Ka2 = 1.2 x 10-15[Ag(NH3)2]+: Kf1 = 2.04 x 103 ; Kf2 = 8.13 x 103
- In developing a method for the determination of formic acid by neutralization volumetry, an analyst calculated the pH as a function of the addition of NaOH for the titration of 30.00 mL of 0.1280 mol/L formic acid with standardized NaOH with concentration of 0.1570 mol/L. With respect to this titration curve, determine the pH of the solution after adding the following volumes of NaOH: 0.00 mL; 10.00 ml; 25 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two decimal places and show your calculations.Calculate the solubility of AgCl(s) in 2.0 M NH3(aq).Ksp = 1.6 × 10-10 for AgClKf = 1.7 × 107 for Ag(NH3)2+(aq) 1.9 × 10-5 M 9.5 × 10-2 M 1.3 × 10-5 M 5.2 × 10-2 M 5.4 × 10-3 Myou want to separate Ni2+ and Mn2+ by precipitating the corresponding sulphidesfrom each other. What pH value must you set so that one of the twometals is precipitated quantitatively (concentration in the solution less than/equal to 10/-5 mol/l)is precipitated while the other is still in solution? Ksp (NiS): 10^-21, Kps (MnS): 10~15; Ks (H2S): 10 ~- 20,Saturation concentration of H2S in water: 0.1 mol/l
- The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant.The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant. Determiner the ff. volume of NaOH used moles of OH- usedA metal M forms a water-soluble hydroxide with a chemical formula of MOH. To determine whatM is, a student prepared 250.0 cm3 of MOH standard solution by dissolving 1.17 g of MOH in distilled water. Then the student titrated 25.0 cm3of the solution with 0.055 M H2SO4(aq) usingphenolphthalein as indicator. The titration was repeated several times and the mean titre was 18.85cm3.(a) Describe how the 250.0 cm3 of MOH standard solution was prepared. (b) (i) Calculate the molar mass of MOH. (ii) Determine what M is. (Relative atomic masses: H = 1.0, O = 16.0) THANKYOU!!!
- 1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…You have performed an iodimetric titration using a commercial vitamin C tablet. Based on the following information below, calculate the %(w/w) of vitamin C(MM=176.16 g/mol) in the tablet: Mass of tablet dissolved in 250.0 mL: 5.422 g Aliquot volume of sample titrated: 25.00 mL Concentration of KIO3: 0.023 M Final burrette volume: 41.31 mL Initial burrette volume: 8.89 mL Blank volume: 0.14 mLA 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was added
