Given:
Concentration of HF = 0.20 m
Volume of HF = 110 ml
Concentration of CsOH = 0.10 m
Volume of CsOH = 440 ml
Ka (HF) = 3.5 x 10^-4
Balanced Chemical Equation:
HF + CsOH ===> CsF + H2O
pH of the solution = log ([acid]/[base]) + pKa
pH = log ([0.20*(110/1000)]/[0.10*(440/1000)]) - log(3.5x10^-4)
pH = 3.15<span />
Answer:
the option e is correct I think
The solution is either saturated or supersaturated with solute
Answer:
to make sure that the source is reliable.
Explanation:
because I am smart
The mercury inside the thermometer is a pure substance hope this helps :)
Group 2, or in the Alkaline Earth Metals section. This is due to the necessity to have a +2 charge to balance out or negate the -2 charge two Bromines carry.
