What is the pH of a 8.6 x 10-8 M solution of HCl(aq) at 25 °C? Report your answer to the hundredths place. Assuming complete dissociation, what is the pH of a 3.98 mg/L Ba(OH)2 solution?Arrange the aqueous solutions from the most acidic to the most basic, at 25 °C. Each value represents a different aqueous solution at 25°C. Acidic Basic each solution as acidic, basic, or neutral.
Calculate the pH of each solution.
Part A [H3O+] = 7.7×10−8 M Express your answer using two decimal
places. pH =
Part B [H3O+] = 7.0×10−7 M Express your answer using two decimal
places. pH =
Part C [H3O+] = 4.2×10−6 M Express your answer using two decimal
places. pH =
Part D [H3O+] = 6.4×10−4 M Express your answer using two decimal
places. pH =
Part E [OH−] = 9.9×10−7 M Express
your answer using two decimal places.
Part...
Calculate pH Using Kw= 1.00X 10^-14 of 0.010 M HCl
Calculate pH Using Ka = 1.75 x 10^-5 of 0.010 M
HC2H3O2
Calculate pH 0.0010 M NaOH
Calculate pH Using Kb= 1.77x 10 ^-5 of 0.010 M
NH3
Calculate pH Using Ka = 1.75 x 10 ^-5 of 0.010 M
NaC2H3O2
Calculate pH Using Kb = 1.77 x 10 ^-5 of 0.010 M
NH4Cl