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- A water sample has exact alkalinity of 220 mg/L CaCO3. The sample contains150.0 mg/L HCO3 at a pH of 7.1 (Temperature = 25 oC).(a) Calculate the carbonate alkalinity in mg/L as CO3.A buffer solution is made that is 0.446 M in CH3COOH and 0.446 M in CH3COONa. (1) If Ką for CH3COOH is 1.80×10-5, what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.095 mol NaOH is added to 1.00 L of the buffer solution. + +A solution consists of 2.0×10-3 M NaHCO3:Calculate the alkalinity (in units of both eq/L and mg/L as CaCO 3) ofthis solution
- 2. The ionization constant for acetic acid is 1.8 x 10-5. How many grams of NaC2H3O2 must be added to one liter of a 0.20 M solution of HC2H3O2 to maintain a hydrogen ion concentration of 6.5 x 10-5 M?A buffer solution is made that is 0.415 M in CH3COOH and 0.415 M in CH3COO- . (1) If Ka for CH3COOH is 1.80×10-5 , what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.103 mol HI is added to 1.00 L of the buffer solution. Use H3O+ instead of H+ .(a) Calculate the pH in the solution formed by adding10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoicacid (C6H5COOH, Ka = 6.3 x 10-5). (b) Calculate the pHin the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.
- What is the pH of a buffer solution prepared by dissolving 0.10 mol of sodium acetate (NaC2H3O2) and 0.2 mol of acetic acid (HC2H3O2) in enough water to give 1.00 L solution? Ka for acetic acid = 1.8 x 10-5 .A 50.00-mL sample of white wine required 24.57 mL of 0.03291M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated.)1. 0.200 M acetic acid is added to water. What is the concentration of H3O* in solution if Kc=1.8x10-6? 2. After an all-night drinking binge, a man pukes 300.0mL of liquid into his trash can. Assuming the puke is 20% HCI and the rest does not affect the pH, what is the pH of the solution resulting from the puke being neutralized with 0.50M NH3? (Kb-1.8x105) 3. If the initial concentration of NH3 is 0.350 M and the concentration at equilibrium is 0.325 M, what is Kc for this reaction?
- bha A buffer prepared by dissolving oxalic acid dihydrate (H2C2O4·2H2O) and disodium oxalate (Na2C2O4) in 1.00 L of water has a pH of 5.333. How many grams of oxalic acid dihydrate (MW = 126.07 g/mol) and disodium oxalate (MW = 133.99 g/mol) were required to prepare this buffer if the total oxalate concentration is 0.241 M? Oxalic acid has pKa values of 1.250 (pKa1) and 4.266 (pKa2).An organic acid (HA) has a molecular weight of 100g/mol, a Kow = 5.6 and a K, = 2.7 x 10-2. If originally 2.0 g of the acid is dissolved in 100 mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100 mL of water, what will be the pH of the water? (Consider the equilibrium processes to be sequential and unrelated chemically) Possible answers: 1.89, 1.48, 2.01, 1.74, 1.61What is the concentration of nitrate ions when 35.00 ml of 0.75 MMg(N0»)2 are diluted to 100.0 ml? How many grams of NaOH (MM = 40.00 g/mol) are needed to make 0.250 L of pH = 10.50 solution? You are titrating 0.0500 L of an unknown solution of NaHS with 0.105 M Ca(OH)2 titr: 20.0 mL of titrant where needed to reach the end point, what was the initial concenti sodium hydrogen sulfate? 2NaHS + Ca(OH), → CaS+ 2H,O +Na,S