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- 8. What mass of solute is needed to prepare each of 1.00 L of 0.125 M K2SO4 solutions? (2 Points) 21.8 g K2SO4 218.0 g K2SO4 2.816 g K2SO4 28.16 g K2SO41. What mass of potassium nitrate KNO3 should be added to 255 g of water to prepare a 15% (m/m) solution of KNO3? [Molar mass KNO3= 101.1 g/mole] 2. Determine the mass of sodium chloride (NaCl) required to prepare a 300 ml Mueller-Hinton broth solution supplemented with 5.5% (wt/vol) sodium chloride solution. [Mwt NaCl = 58.44 g/mol] 3. You have dissolved 45 g of magnesium sulphate in 300 ml distilled water (dH2O). What is the concentration of this MgSO4 solution expressed as % (m/v)? [Mwt MgSO4 = 120.37 g/mol]1. How would you make 10 L of 0.3 M citrate buffer pH 2.5 from solutions of 0.4 M NaCitrate and 0.4 M citric acid? Include the amounts of all components added in mL. pKa = 3.09 2. How many grams of disodium hydrogen phosphate (142 g/mol), mL of 0.5 M HCl or NaOH, and mL of water are needed to make 500 mL of 0.15 M phosphate buffer pH 11.90? What would be the pH of this solution if it were diluted to 2 L with pure water? pKa(1) = 2.15; pKa(2) = 6.86; pKa(3) = 12.38 3. How many mL of 3 M NaOH or 3 M HCl and mL of 0.5 M acetate buffer pH 3.78 do you need to make 600 mL of a 0.02 M acetate buffer pH 5.3?
- 2. Exactly 600.0 mg of pure sodium oxalate, Na,C,0, was dissolved in acid and titrated with a potassium permanganate solution according to the reaction: MnO, + 5C,0, > Mn²+ + CO,. The end point was reached after adding 34.00 ml of titrant. Calculate the molarity of the KMNO, solution.2. A. If 100 mls of 0.03 M HCI is added to 400 mls of 0.5 M glycine buffer at pH 10.4, what is the resultant pH? (pK1 for Gly= 2.2, Pk2=9.4) Gly.4L X.5mol/L= .2 mol HCI.1LX.03mol/L = .003mol Glyº .02mol +.003 mol .023mol [HA] = .023/.5L =.046M, [A-] =.177/.5L = .354M pH = pka +log [A-]/[HA] pH = 9.4 +log.354/.046 = 10.3 [HCI] = [H+] = .003mol/.5L = .006M pH =2.2 Gly + H+ .18mol -.003mol .177mol end start B. What would the pH be if the same amount of HCl as in part A was added to 400 mls of water?1. How many moles of acetate are there in a 200 mL 0.20 M acetate buffer pH 4.95? pKa = 4.76 2. In a solution of pH 4.76, containing both acetic acid and acetate, what can you say about the concentrations of acetic acid and acetate present?
- If your 16x concentrated stock solution contains 20g of NaCl per liter, how much Nacl would one liter of your working solution contain? Round your result to 2 decimal points. g of Nacl1. What is the molality of the following solutions? a. 171.9 g of Sr(NO3)2 is dissolved in 1.44 kg of water. b. 0.883 g of K3PO4 is dissolved in 40.0 g of water. 0.250M=0.250mcl kF IL scl i80.anilio (6250 mcl 0.500M=0.500md wO IL Som1. Calculate the pH of the following solutions: A. [H+] = 1.36 x 10-9 M В. [ОН] —D 3.86 x 10-8 М 2. Calculate the pOH of the following solutions: A. [OH-] = 8.6 x 10-8 M В. рH %3D 3.2 3. What is the pH of a buffer prepared by mixing 100 ml 0.050 mM NAH2PO4 and 25 ml 0.075 mM Na2HPO4? (рКa1%32.2; рКо23 7.21; pКаз312.7)
- 5You just made a 1.5M permanganate solution. What concentration is your potassium permanganate solution in percent? "K: 39.10 g/mole" "Mn: 54.94 g/mole" "O: 16 g/mole" "MW of KMnO4 is 158.04 g/mole" O a. 0.24% Ob. 20.1% O c. 15.8% O d. 23.7% O e. 2%3. Compute for the amount of each component of KCN broth if you were to prepare 280 ml. Express your answers using two decimal places. Follow this format in typing your answers: answerabbreviated unit (e.g. 3.00 g, 0.75 ml, 10.25 mg): Components Amount per liter Polypeptone 3.0 g N22HPO4 5.64 g (Available as NazHPO4 · 7H2O*) Monopotassium phosphate 0.225 g Sodium chloride 0.5% KCN 0.075 g (Available as 10,000 ppm solution) *MW (g/mol): Na-23; P-31; H-1; 0-16 3.3. Monopotassium phosphate /r