You are provided with 0.5M Tris-HCI stock buffer (pH 7.0) and 10% NaCl stock solution. To make 2 liter solution containing 10mM Tris-HCl and 0.9% NaCl, you will need ml of the Tris-HCI stock buffer. Answer: Check 10% sucrose solution is equivalent to mM sucrose solution. The M.W. of sucrose is 342.3 g/mole.

You are provided with 0.5M Tris-HCI stock buffer (pH 7.0) and 10% NaCl stock solution. To make 2 liter solution containing 10mM Tris-HCl and 0.9% NaCl, you will need ml of the Tris-HCI stock buffer. Answer: Check 10% sucrose solution is equivalent to mM sucrose solution. The M.W. of sucrose is 342.3 g/mole.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter24: The Standardization Of A Basic Solution And The Determination Of The Molar Mass Of An Acid

Section: Chapter Questions

Problem 3ASA: A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to...

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The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.500 moles of a monoprotic weak acid (?a=8.9×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point? pH= ( Please type answer note write by hend )
What is the component concentration ratio, [Pr−]/[HPr], of a buffer that has a pH of 4.98?(Ka of HPr = 1.3 × 10−5) Report your answer to 3 significant figures.
A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?
An automatic titration of Cola product was analyzed and the following results were produced: Volume of Standardized NaOH Titrant used to achieve the first equivalence point in titration: Trial #1: 1.300 mL Trial #2: 1.137 mL Trial #3: 1.140 mL May you explain why trial #1 was skewed; for example, if pipetting of the 25.00 mL was done incorrectly, how would the molarity change if the volume examined was supposed to be 24.50 mL?
You are asked to prepare 500. mL 0.300 M acetate buffer at pH 5.10 using only pure acetic acid (MW=60.05 g/mol, p?a=4.76), 3.00 M NaOH, and water. How many grams of acetic acid will be needed to prepare the 500. mL buffer? Note that the given concentration of acetate refers to the concentration of all acetate species in solution. What volume of 3.00 M NaOH, must be added to the acetic acid to achieve a buffer with a pH of 5.10 at a final volume of 500. mL? Ignore activity coefficients.
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.
How many grams of sodium fluoride should be added to 40.0 mL of 0.223 M hydrofluoric acid solution to produce a buffer of pH 4.70 with a total diluted volume of 500. mL? The Ka for hydrofluoric acid is 7.20x10-4. Group of answer choices 0.0103 g 0.129 g 13.6 g 27.2 g 170. g
A buffer is made up of equal volumes (468.3 mL of each) of 0.860 M A H and 0.884 M A minus. 29.32 mL of 0.399 M N a O H is added to the buffer. How many moles of A minus are present after the addition of N a O H? Please use correct significant figures. Answer: (0.426) (mol)
10.Calculate the pH of the solution prepared by dissolving 0.48 mol of NH3(Kb=1.77x10-5) and 0.750 mol of ammonium chloride in enough water to make 1.00L of buffer solution Group of answer choices A, 5.09 B, 9.05 C, 9.44 D, no correct answer E, 10.1 11,The equivalence point of titrating of the weak base with the strong acid will be observed at Group of answer choices A, pH>7 B, pH<7 C, pH=pKb D, pH>pKb E, pH=7 12,The titration curve of titrating a diprotic acid with a strong base will have two distinct equivalence points Group of answer choices A, if Ka1<<Ka2 B, if Ka1=Ka2 C, always D, in case of ta strong acid E, if Ka1>>Ka2
Common-ion effect What is the solubility (in grams per liter) of strontium sulfate, SrSO4, in 0.20 M sodium sulfate, Na2SO4? Kspof SrSO4 = 2.5x10-7 show solution and explain
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.
A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol