In an acid$-$base reaction, both acid and base must be present because an acid cannot

lose a proton unless a base is present to accept it$.$ Given the Ka values of the

following compounds: trifluoroacetic acid $($CF$3$COOH$),$ Ka $=5\mathrm{.}62$x$10-1$

; acetic acid

$($CHJCOOH$),$ Ka $=$ l$\mathrm{.}75$xto$5$

; methyl alcohol $($CH$30$H$),$ Ka $=3\mathrm{.}2$xl$0-16$

; nitric acid

$($HN$03),$ Ka$=28.$

i$)$Calculate the pKa value of each of the given compounds.

ii$)$Arrange those compounds from strongest to weakest acid and write your reason.

iii$)$ By comparing the conjugate base of those acids, arrange from the strongest to the weakest base, and write your reason.

iv$)$ Predict the product of an acid$-$base reaction between nitric acid $($HN$03)$ and methyl alcohol $($CH$30).$

v$)$ Calculate at what pH is the concentration of acetic acid $($CH$3$COOH$),10$

times greater in its acidic form than basic form?