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How many grams of solid KH2PO4 (MW=136 g/mol) and solid K2HPO4 (MW = 174 g/mol) would you use to prepare a 1.00 L of a 0.500 M phosphate buffer at pH = 6.8.[pKa for KH2PO4 = 7.2]
What will be the pH if 5.00 grams of solid KOH is added to 500 mL of a solution containing 0.020 moles of HCl?
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- 500 mL of a buffer solution contains 0.050 mol NaHSO3 and 0.031 mol Na2SO3. (pKa = 7.172). What is the pH of the buffer? Write the net ionic equation for the reaction that occurs when NaOH is added to this buffer. Determine the pH of the buffer solution after 10 mL 0.1 M NaOH has been added.A 1.7483-g sample containing Al(NO3)3, AlCl3, and inert material was dissolved in acid and divided into two equal portions. One portion was treated with 5.00 mmol of AgNO3. The excess Ag+ required 28.89 mL of 0.l002 M KSCN for titration. The other portion required 26.02 mL of 0.1193 M NaOH for titration:Al3+ + 3 OH- → Al(OH)3(s)Calculate the percentage composition of Al(NO3)3 and AlCl3 in the sample.Calculate the volume, in milliliters, of a 0.770 M KOH solution that should be added to 5.000 g of HEPES (MW = 238.306 g/mol, pKa = 7.56) to give a pH of 7.50. KOH volume = mL
- Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 16.15 mL of 0.250 M NaOH to reach the phenolphthalein end point. Which of the following chemical equations represents the reaction between acetic acid and sodium hydroxide? a.CH3COOH + NaOH ---> CH3COO - + NaOH2 + b. CH3CH2OH + NaOH --> CH3CH2O - + NaOH2 + c. CH3COOH + NaOH --> CH3COONa + H2O d. CH3CH2OH + NaOH --> CH3CH2Na + H2OA sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 84.3-mL sample of this solution was withdrawn and titrated with 0.0948 M HBr. It required 64.6 mL of the acid solution for neutralization.(a) What was the molarity of the Ca(OH)2 solution? M(b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution? g/100mLIf a sample of silver coin weighing 0.5230 g gives a precipitate of AgCl (143.45) weighing 0.3559 g, the weight of AgBr (187.90) that could have been obtained from the same weight of sample is 0.89 grams. true or false?
- A mixture containing only KCl (74.55 g/mol) & NaBr (102.89 g/mol) was analyzed by the Mohr method. A 0.50 g sample which was dissolved in 50 mL of water and treated with 0.500 mL of 0.0010 M sodium chromate, required 10 mL of 0.50 M AgNO3 for complete titration. AgCl FW=143.32 g/mol , AgBr FW=187.77 g/mol what is suitable indicator?a. Na2CrO4b. AgNO3c. phenolphthaleind. any of these can be usedexpected endpoint?a. pink precipitateb. red solutionc. red precipitated. any of these is possiblewhat is %w/w KCl and %w/w NaBr?What is the pH of a buffer that results when 500 mL of a 3.00 M solution of H3PO4 is mixed with 500 mL of a 8.00 M solution of NaOH and diluted with water to 3.50 L?How many grams of solid KH2PO4 (MW=136 g/mol) and solid K2HPO4 (MW = 174 g/mol) would you use to prepare a 1.00 L of a 0.500 M phosphate buffer at pH = 6.8.[pKa for KH2PO4 = 7.2]
- 0.28g 0f MBr is dissolved in distilled water and made up to 250mL mark in a volumetric flask. 25 mL of this solution is titrated against 0.019 M silver nitrate solution using eosin as indicator. The end point was obtained at 12.4 mL of AgNO3 solution . Calculate the molar mass of the metal bromide.(5) a) A nitrous acid/sodium nitrite buffer solution is prepared. 20.0 mL of 6.50 M nitrous acid (HNO2) and 8.52 g of sodium nitrite (NaNO2, molar mass 68.99 g/mol) are placed in a 250. mL volumetric flask. The flask is filled to the mark with water and inverted 10 times to mix thoroughly. What is the pH of this buffer? Take Ka for Nitrous Acid to be 4.52 x 10-4. pH: b) 2.00 mL of a 2.50 M solution of NaOH is added to 75.0 mL of the buffer prepared above. What is the pH of this solution? How much did the pH change? pH: change in pH: c) What is the pH of pure distilled water (just give the pH, no calculations are necessary). d) If 2.00 mL of 2.50 M…How many grams of solid KH2PO4 (MW=136 g/mol) and solid K2HPO4 (MW = 174 g/mol) would you use to prepare a 1.00 L of a 0.500 M phosphate buffer at pH = 6.8.[pKa for KH2PO4 = 7.2] What will be the pH change if you add 5.00 grams of solid KOH (MW=56.11 g/mol) to the above buffer?
