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Super Ninja has a 10.00 mL sample of 0.15 M of chlorous acid, HClO2(aq).
- This acid is titrated with 0.20 M sodium hydroxide, NaOH. Calculate the pH at equivalence point.
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- Calculate the mass of sodium acetate, NaCH3COO, you should add to 500. mL of a 0.150-M solution of acetic acid, CH3COOH, to buffer a solution at a pH of 4.57.A solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of solution. A 30.00-mL sample of the solution is titrated with 0.272 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.0.800 grams of solid barium hydroxide, Ba(OH)2, is added to enough water to prepare 250.0 mL of solution. Calculate the pH of the resulting solution.
- What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml of 3.66M Sodium Formate (NaHCO2) together? If you were to now add 18 ml of 1.2M NaOH to the buffer solution, what would the new pH be?0.800 grams of solid barium hydroxide, Ba(OH)2, is added to enough water to prepare 250.0 mL of solution. Calculate the pH of the resulting solution. AnswerCalculate the pH of a solution formed by adding 5.00 grams of solid sodium formate, NaCHO₂, to 180.0 ml of 0.220 M formic acid solution, HCHO₂. You may assume that the salt dissolves completely and that the change in volume is negligible upon addition of the solid.
- Acid rain is due to the dissolution of sulfur oxide (SO3) present in contaminated areas in the droplets of water giving rise to sulfuric acid (H2SO4). If the concentration of H2SO4 that originated in the drops is 3 x 10-4 M, what would the pH of the rain be?Calculate the pH of a solution formed by adding 6.00 grams of solid sodium formate, NaCHO₂, to 200.0 ml of 0.400 M formic acid solution, HCHO₂. You may assume that the salt dissolves completely and that the change in volume is negligible upon addition of the solid.pH = ___A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph above. What is a pH value between 2.5- 7.5 where the concentration of the weak acid being titrated is less than the concentration of its conjugate base?
- 1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?A solution is formed by adding 2.70 grams of solid sodium hypochlorite, NaClO, to 200.0 ml of 0.0210M calcium hypochlorite, Ca(ClO)₂. Calculate the pH of the resulting solution. You may assume that the sodium hypochlorite dissolve completely and that the change in volume is negligible with the addition of the solid.If 10 mL of 0.1 M hypothetical acid, HA, is added with 10 mL of 0.1 M of the salt of its conjugate base, XA, what is the pH of the solution?
