1. You will use 0.5mM PNPP, 0.2M Tris-HCl, and 1mM P; stock solutions to prepare two sets of fivesamples (Sets A and B), each with varying P; concentrations. The PNPP concentration for allsamples in Set A will be 0.05mM; and 0.150mM for all samples in Set B.Fill out the tables below and use them to prepare your samples. Be aware of the following:• Prepare the samples directly in cuvettes. Prepare one sample at a time to minimizeexposing PNPP to air. You can prepare the next sample while the current one is beingmeasured.• Each sample before adding enzyme (i.e., the cuvette only contains PNPP, Pi, and Tris-HCI)is its own blank. In other words, you add the appropriate amounts of PNPP, Pi, and Tris-HCI to a cuvette, press "Measure Blank", then add 100μL of AP to the same cuvette, mix,and press "Measure Sample".•You must blank the instrument (before adding the enzyme) each time you prepare a newsample.Table 1. Sample Set A (PNPP concentration = 0.05mM)Final [Pi](μM)Vol of 1mM Pi(μL)[PNPP](mM)Vol of 0.5mM PNPP(μL)Vol of 0.2M Tris-HCI(μL)Vol of enzymeTotal Vol(μL)(μL)00.0510015003.330.051001500200.051001500500.0510015001000.051001500

Final [Pi] ([Pi]2) (uM)Vol of 1 mM Pi(Va)(uL)[PNPP] ([PNPP]2)(mM)Vol of 0.5 mM PNPP(Vb)(uL)Vol of…

Answered: 1. You will use 0.5mM PNPP, 0.2M…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. A solution was prepared by adding 4.95 g sodium acetate (NaC;H;O2) to 250.0 mL of 0.150 M acetic acid (K = 1.75 x 10). Assume negligible volume change. a) What is the pH of the resulting solution? PH: pk2 + log CH3 02) moles saium 4.959 0.06 mol %3D 2cent %3D 82gmu H: -log (1.73x 10) + log 0.24 moles 2cete 250 x 0.15 IL :00375 1000me PH : 4 1.96 O.06 (N2 G Hs0): 0.24m 0.230 L O.0375 : CCHS COOH): 0 15 m Assume 125.0 mL of the solution prepared above was put into a beaker and 82 mg of NaOH was added to it. What is the pH of this new mixture? b)
6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH3CO2H) to 1.00 L H,0. What is the pH of the solution at equilibrium? (K, = %3D 1.8 x 10°)
Calculate the percentage CH3COOH in a sample of vinegar from the following data.Sample = 15.00 g, NaOH used = 43.00 ml ; 0.600 N H2SO4 used for back titration =0.250 ml ; 1.00ml NaOH is equivalent to 0.0315 g H2C2O4. 2H2O.
3.A sample is known to contain NaOH, NA2CO3 NaHCO3 or compatible mixture of these together with inert matter. With methyl orange, a 1.100 g sample requires 31.40 mL of HCI ( 1.00 mL is equivalent to 0.0140g CaO). With phenolphthalein indicator, the same weight of sample requires 13.30mL of the acid. What is the percent composition of the sample?
Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12
A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2 (ethylamine), the burette is filled with 0.20 M HCl as titrant. Kb of C2H3NH2 = 6.5 ´ 10-4 What is the initial pH of above sample solution before titration starts?
V A solution is prepared at 25 °C that is initially 0.27M in chloroacetic acid (HCH₂CICO₂), a weak acid with K=1.3 × 10-³, and 0.48M in sodium chloroacetate (NaCH₂CICO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. -3 pH = 1 X Ś
4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.
A solution is made by dissolving 0.111 moles of N2H4 (Kb = 3.0 x 10-6 ) and 0.199 moles of N2H5Cl in water and diluting to 1.00 L. What is the pH of the resulting solution?
An intrinsic property is one a That is dependent on how much of the material is present That is analogous to the flammability of any substance That is analogous to the flammability of any substance That only changes withaltitude How many moles are in 20 mg of steric acid, CH_3(CH_2)_{16}COOH?
Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. 1 3 4 NEXT > Two solutions are mixed: 40.0 mL of 0.500 M NH3 and 25.0 mL of 0.300 M HCI. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. Before (mol) Change (mol) After (mol) -0.0075 Initial (M) Change (M) Equilibrium (M) E 0.313 - x 0 0.0100 0 0.500 + x 40.0 0.115 + x NH3(aq) -0.0100 NH3(aq) + 0.500 2 0.500 - x 0.115-x 0.500 2 0.0125 : on by constructing a BCA table, constructing an ICE table, ant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. -■· 0.300 +
A solution is prepared at 25 °C that is initially 0.46M in propanoic acid (HC,H,CO,), a weak acid with K,= 1.3 x 10 - 5 and 0.15M in sodium propanoate (NaC,H,CO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH

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