An acid HA has a vapor density of 5.11 g/L at 25 °C and 1.00
atm. When 1.50 g of HA is dissolved in enough water to make 100.0
mL of solution, the pH is found to be 1.80. Calculate K
for the acid.
An acid HA has a vapor density of 5.11 g/L at 25 °C and 1.00 atm....
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee-cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. A 0.704 g of a pure acid, HA, is dissolved in water and an acid-base...
1. A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is dissolved in enough water to obtain a 300 mL solution, the pH of the resulting solution is found to be 2.62. What is the value of Ka for this acid? 2. A weak monoprotic acid has pKa = 3.08. Calculate the percent ionization of a 0.35 M solution of this acid. 3. Calculate the pH of a solution that is 0.050 M in CH3COOH...
We place 0.134 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.18 . Calculate the ionization contant, Ka, of HA
We place 0.133 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.23 . Calculate the ionization contant, Ka, of HA.
We place 0.118 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.29 . Calculate the ionization contant, Ka, of HA.
Question 1 HA is a weak acid. Its ionization constant, Ky, is 5.1 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.053 M. Question 2 We place 0.134 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.18. Calculate the ionization contant, K. of HA. Question 3 We place 0.577 mol of a weak acid, HA, and 13.6 g of...
The vaporization of 1 mole of liquid water (the system) at 100.9°C, 1.00 atm, is endothermic. H2O(l)+40.7kj -------> H2O(g) Assume that at exactly 100.0°C and 1.00 atm total pressure, 1.00 mole of liquid water and 1.00 mole of water vapor occupy 18.80 mL and 30.62 L, respectively. Part 1 Calculate the work done on or by the system when 1.25 mol of liquid H2O vaporizes. Part 2 Calculate the water's change in internal energy
At 298 K and 1.00 atm, assume that 22 mL of NO gas reacts with 16 mL of oxygen gas and excess water to produce gaseous nitric acid according to the following equation: 2 N O ( g ) + 3/2 O 2 ( g )+ H 2 O ( l )= 2 H N O 3 ( g ) . If all of the nitric acid produced by this reaction is collected and then dissolved...
Determine the vapor pressure (in atm) , at 25.0 o C, of an aqueous Glycerin (C3H8O3) solution that is formed by adding 75.0 g C3H8O3 to enough water to make 563 mL solution. Density solution = 1.05 g/mL Vapor pressure H2O @ 25oC = 23.76 torr
We place 0.612 mol of a weak acid, HA, and 12.9 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.42 . Calculate the ionization constant, Ka, of HA.