Q6. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 86.4 mL of
0.494 M H2SO4. Calculate the
mass of solid BaSO4 formed and the pH of the mixed solution
Q6. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 86.4 mL of 0.494 M...
Be sure to answer all parts. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 76.2 mL of 0.450 M H2SO4. Calculate the mass of BaSO4 formed. g Calculate the pH of the mixed solution.=
Check my work Be sure to answer all parts. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 81.0 mL of 0.375 M H2S04. Calculate the mass of BaSO4 formed. Calculate the pH of the mixed solution.
Check my work Be sure to answer all parts. A student mixes 50.0 mL of 1.00 M Ba(OH), with 81.0 mL of 0.375 M H,SO. Calculate the mass of BaSO4 formed. 7.10 Calculate the pH of the mixed solution. 10.5 ®
50.0 mL of 1.00 M Ba(OH)2 is mixed with 81.6 mL of 0.450 M H2SO4. Calculate the pH of the solution after BaSO4 precipitates. 1.00 13.31 13.00 0.69 13.88
calculate the mass in grams of BaSo4 that was formed from the following information. Moles of Ba(OH)2 = Moles BaSo4 volume Ba(OH)2 dispensed = 10 ml Molarity of H2SO4 used = 0.100 M Molarity of Ba(OH)2 solution = 0.118 M
In a constant pressure calorimeter 50.0 mL of 0.310 M Ba(OH)2 was added to 50.0 mL of 0.620 M HCl. the reactions caused the temperature of the solution to rise from 23.77 c to 27.99 c if the solution has the same density and same specific heat as water (1.00 g/mL and 4.184 j/g c ) what is triangle H for this reaction (per mole of H2O produced) assume that the total volume is the sum of the individual volumes
In a constant-pressure calorimeter, 50.0 mL of 0.350 M Ba(OH)2 was added to 50.0 mL of 0.700 M HCl. The reaction caused the temperature of the solution to rise from 24.49 C to 29.26 C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g• C) respectively), what is ?H for this reaction (per mole H2O produced)? Assume and the total volume is the sum of the individual volumes. ?H= _______ kJ/mol H2O
Two solutions, 50.0 mL of 1.00 M BaCl2 (aq) and 50.0 mL of 1.00 M Na2SO4 (aq), both at 21.5 ° C, are mixed in a thermometer. The heat capacity of the thermometer with the solutions in is 1.23 kJ / ° C. During mixing, the temperature of the solution rises to 23.4 ° C. How much heat (qrxn) is released from the reaction that occurs when 1 mole of BaSO4 (s) is precipitated? Give the answer in kJ.
In a constant-pressure calorimeter, 50.0 mL of 0.340 M Ba(OH), was added to 50.0 mL of 0.680 M HCI. The reaction caused the temperature of the solution to rise from 22.91 °C to 27.54 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g • °C,) respectively), what is AH for this reaction (per mole H,O produced)? Assume that the total volume is the sum of the individual volumes.
4.82 (a) How many milliliters of 0.120 M HCI are needed to com- pletely neutralize 50.0 mL of 0.101 M Ba(OH)2 solution? (b) How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.200 g of NaOH? (c) If 55.8 mL of a BaCl2 solution is needed to precipitate all the sulfate ion in a 752-mg sam- ple of Na2SOs, what is the molarity of the BaCl2 solution? (d) If 42.7 mL of 0.208 M HCl solution is needed...