15. the pAg during the titration of 50.0 ml of 0.040 M NaCl with 20 ml of 0.100 AgNO3 (Ksp for AgCI=1.82×10-10) a. 4.87 b. 3.87 C. 2.76 d. 4.95 e. 2.85 fer addition of indicator the solution needed 15.46 ml of Coca is 100.08
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- A 370.00 mL solution of 0.00185 M A3B4 is added to a 390.00 mL solution of 0.00100 M C3D4. What is pQsp for A3D4?Chemistry A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this solution is taken and titrated with 0.05 M EDTA at pH = 10 in the presence of Erio – T indicator, the consumption is found as 12 mL. A new 10 mL was taken from the same solution and (NH4)2C2O4 is added on it and then formed the precipitate is filtered. The filtered solution is titrated with the same EDTA solution and the consumption is found as 3 mL. So find the Ca2+ and Mg2+ amounts in the main sample solution in terms of mg/L.Tony is showing a bacterium having high pH requirement for its growth. He then has to prepare a minimal medium at pH 9. Adding 0.5 ml of the pH indicator to 10 ml of the medium, the solution remained colorless. The pH of the medium was adjusted using 2.25 ml of the 0.05 N titrant. a. What was the pH indicator utilized? b. What is the amount of 1 N titrant needed to adjust 150 ml of minimal medium to pH 9? c.What was the titrant he used?
- A biochemist needs 750 mL of an acetic acid–sodiumacetate buffer with pH 4.50. Solid sodium acetate(CH3COONa) and glacial acetic acid (CH3COOH) areavailable. Glacial acetic acid is 99% CH3COOH by massand has a density of 1.05 g/mL. If the buffer is to be 0.15 Min CH3COOH, how many grams of CH3COONa and howmany milliliters of glacial acetic acid must be used?4. The molar absorptivities of the indicator weak acid HIn (K_{a} = 1.42 * 10 ^ - 5) and its conjugate base In at 570 were determined as epsilon(HIn) = 7120 and ε(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 and pH = 6.5 .The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.
- A 1.0-LL buffer solution contains 0.100 molHC2H3O2molHC2H3O2 and 0.100 molNaC2H3O2molNaC2H3O2. The value of KaKa for HC2H3O2HC2H3O2 is 1.8×10−51.8×10−5. Calculate the pHpH of the solution upon addition of 21.4 mLmL of 1.00 MHClMHCl to the original buffer. Express your answer using two decimal places.Which of the following statements is advantageous? A). The main differences between potentiometric and conductometric titrations are that potentiometric titrations exemplify the analyte sample-by-sample while conductometric titrations show the potential of the analyte B). A conductivity is analyl from the people of the charge. C.) Conductivity increases rapidly as close as equivalence, as a strong acid and a strong base will decrease D). The conductor remains constant according to the viscosity of the pixel, the decomposer and its size, which consists of design modelling.A laboratory manager wants to prepare 500.00 mL of a buffer with a pH of 4.471 from equimolar solutions of CH3CO2H (Ka = 1.800e-5) and LiCH3CO2. What volume of the LiCH3CO2 solution would be required? Key Concept: Buffers resist pH change and are prepared by mixing the conjugate acid and base together. The pH is determined from the Henderson-Hasselbach equation: pH = pKa + log([A−]/[HA]).Solution: Since the molarities of the two solutions making the buffer are the same, the Henderson-Hasselbach equation can be written as: pH = pKa + log(V(A−)/V(HA)) where V(A−) = the volume of the conjugate base and V(HA) = the volume of the conjugate acid.
- The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8, respectively. Which one would be more suitable for use in asolution buffered at pH = 7.0? What other substances would be needed to makethe buffer?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 mLApproximately 6 mL of conc. perchloric acid ( 72% ) was transferred to a bottle and diluted with about 1 liter of water. A sample containing 251.5 mg of primary standard Na2B4O7.10H2O (Fwt= 382g/mol) required 27.41 mL of the HClO4 solution to reach the methyl red end point. What is the molar concentration of the HClO4 solution? Na2B4O7.10H2O + HClO4 ------------> NaClO4 H2B4O7.10H2O