Identify which indicator will be suitable for the following titrimetric analyses: a. 0.100 M solution of HOAC (K, = 1.78 x 10 ) with 0.100 M NaOH. b. 0.0527 M solution of NH,CI (K, = 1.80 x 105) with 0.100 M NaOH. c. 0.0162 M solution of piperidine hydrochloride (K, 1.60 x 10³) with 0.100M NAOH. d. 0.350 M solution of NaOAC (K, = 1.78 x 105) with 0.200 M HCI. e. 0.0568 M solution of sodium dichloroacetate (Ka = 3.32 x 102) with 0.200 M HCI. %3D
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- 1. An instrument used to measure the acidity or alkalinity of a solution. 2. Chemicals of high purity which are used to standardize a solution 3. Used as standard but have a tendency to lose water from crystallization.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,…Suppose that you want to titrate a sample of vinegar with standard sodium hydroxide solution to determine the concentration of acetic acid in it, and you want to use an indicator to help you determine the end-point. Which of the following indicator would be suitable? (A) Bromocresol Green (Ka ~ 2.0 x 10–5; color: yellow in acid; blue in base) (B) Methyl Red (Ka ~ 5.0 x 10–6; color: red in acid; yellow in base) (C) Bromothymol Blue (Ka ~ 6.0 x 10–8; color: yellow in acid; blue in base) (D) Any of them
- Q: The solubility product of Zn(OH)2 at 25oC is 3.0 x 10-6 M3. Calculate the solubility of Zn(OH)2 in water in gdm-3. [Ar: Zn = 65.5; O = 16; H = 1] The Mr for Zn(OH)2 is 99.5. When I multiply it with Ksp, I didn't get the same answer as the given answer which is 0.904 gdm-3.1.Which of the following substances have a solvatochromic property? a.potassium hydrogen phthalate b.sodium carbonate c.sodium bicarbonate d.bromocresol green 2.If the pKa of the indicator is approximately 6, to which of the following equivalence point will it be most suitable? a.pH 10 b.pH 13 c.pH 4 d.pH 53. Referring to the figure below, what volume of the titrant was used to reach half-neutralization equivalence point? a.25 mLb.20 mLc.50 mLd.56 mLPhenolphthalein, a colorless weak acid (Ka = 6.31 x 10^-10) which dissociates in water forming pink anions is widely considered a suitable indicator for this titration. Along with a suitable calculation, find the working/useful range of this indicator to explain its use.
- Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3Use the following solubility data to calculate a value of Ksp for each compound: a) CdCO3 : 1.0 x 10^-6 M b) Ca(OH)2 : 1.06 x 10^-2 M c) PbBr2 : 4.34 g/L d) BaCrO4 : 2.8 x 10^-3 g/LCalculate 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 M
- An ecobotanist separates the components of a tropical barkextract by chromatography. She discovers a large proportion ofquinidine, a dextrorotatory isomer of quinine used for control of arrhythmic heartbeat. Quinidine has two basic nitrogens (K(b1)=4.0X10⁻⁶ and K(b2)=1.0X10⁻¹⁰). To measure theconcentration, she carries out a titration. Because of the low solubility of quinidine, she first protonates both nitrogens withexcess HCl and titrates the acidified solution with standardized base. A 33.85-mg sample of quinidine (M=324.41g/mol) isacidified with 6.55 mL of 0.150 MHCl.(a) How many milliliters of 0.0133 MNaOH are needed to titrate the excess HCl?(b) How many additional milliliters of titrant are needed to reach the first equivalence point of quinidine dihydrochloride?(c) What is the pH at the first equivalence point?an ecobotanist separates the components of a tropical barkextract by chromatography. She discovers a large proportion ofquinidine, a dextrorotatory isomer of quinine used for control of arrhythmic heartbeat. Quinidine has two basic nitrogens (K(b1)=4.0X10⁻⁶ and K(b2)=1.0X10⁻¹⁰). To measure theconcentration, she carries out a titration. Because of the low solubility of quinidine, she first protonates both nitrogens withexcess HCl and titrates the acidified solution with standardized base. A 33.85-mg sample of quinidine (M=324.41g/mol) isacidified with 6.55 mL of 0.150 MHCl.(c) What is the pH at the first equivalence point?What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M with respect to each ion? In some cases it may be necessary to control the pH. (Hint: Consider the Ksp values given in Appendix J.) (a) Hg22+ and Cu2+ (b) SO42− and Cl– (c) Hg2+ and Co2+ (d) Zn2+ and Sr2+ (e) Ba2+ and Mg2+ (f) CO32− and OH–