molarity = weight of substance * 1000/gram molar mass * volume of solution in ml
= 21*1000/84*480 = 0.52M
molarity = weight of substance * 1000/gram molar mass * volume of solution in ml
= 57*1000/98*220 = 2.64 M
21.0 g NaHCO_3 in 480.0 mL solution 57.0 g H_2SO_4 in 220.0 mL solution M =
A student has 480.0 mL of a 0.1140 M aqueous solution of CoCl2 to use in an experiment. She accidentally leaves the container uncovered and comes back the next week to find only a solid residue. The mass of the residue is 9.076 g. Determine the chemical formula of this residue.
Calculate the pH when 57.0 mL of 0.237 M perchloric acid is mixed with 57.0 mL of 0.237 M sodium hydroxide solution at 25 °C. Calculate the pH when 57.0 mL of 0.237 M of a certain monoprotic weak acid, HA, is mixed with 57.0 mL of 0.237 M sodium hydroxide solution at 25 °C. For HA, the Ka is 8.1× 10–5.
When 22.00 mL of 0.5000 M H_2SO_4 is added to 22.00 mL of 1.000 M kOH in a coffee-cup calorimeter at 23.50 degree C, the temperature rises to 30.17 degree C. Calculate delta H of this reaction. (Assume that the total volume is the sum of the individual assumes and that the density and specific heat capacity of the solution are the same for pure water.) (d for water = 1.00 g/mL; c for water - 4.184 J/g degree C.)...
Calculate the mass/volume percent (m/v) of 21.0 g NaCl in 67.5 mL of solution.
Calculate the pH at 25°C of 220.0 mL of a buffer solution that is 0.350 M NH4Cl and 0.350 M NH3 before and after the addition of 2.40 mL of 6.0 M HNO3. (The pKa for NH4+ = 9.75)
Suppose 0.591 g of zinc iodide is dissolved in 50. mL of a 57.0 m M aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it Round your answer to 2 significant digits. M M10 ? X
A 90.0-mL sample of 1.00 M NaOH is mixed with 45.0 mL of 1.00 M H_2SO_4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 23.7degreeC. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.5degreeC. Assume that the density of the mixed solutions is 1.00 g/mL, that the...
A 12.0 mL sulfuric acid solution, H_2SO_4(aq), was titrated using 0.250 M KOH. If the complete neutralization of the acid required 18.6 mL of the KOH solution, what was the molarity of sulfuric acid? Answer. 0.775 M
Calculate the pH of the resulting solution if 21.0 mL of 0.210 M HCl (aq) is added to 31.0 mL of 0.210 M NaOH(aq) pH Calculate the pH of the resulting solution if 21.0 mL of 0.210 M HCl(aq) is added to 11.0 mL of 0.310 M NaOH(aq) pH II
A chemist titrates 220.0 mL of a 0.7177 M ethylamine (C2HzNH) solution with 0.5582 M HCl solution at 25 °C. Calculate the pH at equivalence. The pK, of ethylamine is 3.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = 0 1 x 6 ?