Consider a buffer solution consisting of $0\mathrm{.}40$ M NaCNO and $0\mathrm{.}40$ M HCNO, which has an initial pH of $3\mathrm{.}46.$ Ka for HCNO $=3\mathrm{.}5$ x $104.$ If $10.$ mL of a $2\mathrm{.}0$ M NaOH solution are added to $1\mathrm{.}0$ L of this buffer, select the options that correctly reflect the steps required to calculate the change in pH$.$ Select all that apply. pHnew $=$log$(3\mathrm{.}5\backslash$times $104\backslash$times $0\mathrm{.}420\mathrm{.}38)=3\mathrm{.}41$

$[$H$3$O$+]$new $=3\mathrm{.}5$ x $104$ x $0\mathrm{.}380\mathrm{.}42$

pHnew $=$log$(3\mathrm{.}17$ x $104)=3\mathrm{.}50$

$[$H$3$O$+]$new $=3\mathrm{.}5$ x $104$ x $0\mathrm{.}420\mathrm{.}38$

Ka$,$ new $=[$H$3$O$+]$new$[$CNO$]$new$[$HCNO$]$new

$=3\mathrm{.}17$ x $104$