Use the References An aqueous solution of trichloroacetic acid, that is 3.00 percent by weight trichloroacetic acid, has a density of 1.0133 g/mL. A student determines that the freezing point of this solution is -0.611 °C. Based on the observed freezing point, what is the percent ionization of the acid and the value of Ka? K for H₂O is 1.86 °C/m. % ionized- K₂ W

Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Be sure each entry you write includes the correct number of significant digits. [4,0°] solution pH x10 12 A 2.1 х 10 mol/L ||mol/L 6.57 В C 0.77 mol/L

When the CaSO4 is 2.4 x 10^-5 what would be the volume of H2O to dissolve .33g of CaSO4

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type (check all that apply) effect of change on pH (check one) solution initial components change acidic pH higher Н,О, КОН add HNO3 рH lower A basic neutral pH the same acidic pH higher Н, О, КОН add KNO3 рH lower В basic neutral pH the same acidic pH higher H,0 basic add HCl pH lower neutral pH the same acidic pH higher D H,O basic add NaCl рH lower neutral pH the same O OlO O