The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10-6 mol/L when about a tenth of a mole of the acid is dissolved in a liter of water. acid H CI HCIO ΗΝΟ, H₂S strong or weak? strong weak strong weak species present at 10-6 mol/L or greater when dissolved in water 0 0 X S

In an aqueous solution, if H+ increases then OH decreases. True O False

Determine the [OH−], pH, and pOH of a solution with a [H+]of 5.7×10−9 M at 25 °C. [OH−]=     pH=     pOH=     Determine the [H+] , pH, and pOH of a solution with an [OH−] of 5.1×10−9 M at 25 °C. [H+]=   MM pH=     pOH=     Determine the [H+] , [OH−] , and pOH of a solution with a pH of 3.063.06 at 25 °C. [H+]=     [OH−]=     pOH=     Determine the [H+][H+] , [OH−][OH−] , and pH of a solution with a pOH of 5.525.52 at 25 °C. [H+]=     [OH−]=     pH=

The H⁺ concentration in an aqueous solution at 25 °C is 3.7 × 10⁻⁴. What is [OH⁻]?

Determine the [OH−] , pH, and pOH of a solution with a [H+] of 0.0096 M at 25 °C.[OH−]=  MpH=pOH=Determine the [H+] , pH, and pOH of a solution with an [OH−] of 7.5×10−7 M at 25 °C.[H+]=  MpH=pOH=Determine the [H+] , [OH−] , and pOH of a solution with a pH of 12.84 at 25 °C.[H+]=  M[OH−]=  MpOH=Determine the [H+] , [OH−] , and pH of a solution with a pOH of 4.34 at 25 °C.[H+]=  M[OH−]=  MpH=

Classify each of the following substances as either a strong or weak acid, strong or weak base, or a soluble or insoluble salt. Clear All strong acid ВаBr, weak acid HI strong base NAOH weak base HCN soluble salt Ba(OH)2 insoluble salt

Calculate the percent ionization of a 0.437 M solution of hypochlorous acid. (Assume that K₁ (HClO) = 3.5 × 10−8.) % lonization = %

Calculate the hydroxide ion concentration of an aqueous solution of 0.480 M hydrofluoric acid. (Assume that K₂ (HF) = 7.2 × 10−4.) [OH] =| M

The H⁺ concentration in an aqueous solution at 25 °C is 4.5 × 10⁻⁴. What is [OH⁻]?

Each value represents a different aqueous solution at 25 °C. Classify each solution as an acid, base, or neutral. [OH−]= 3.0 × 10 − 6 [H+]= 8.1 × 10 − 13 pOH= 13.67 pOH= 7.00 [H+]= 5.3 × 10 − 3 [OH-]= 3.0x 10^-6 is a(n) Question Blank 1 of 5 , [H+]= 8.1 x 10^-13 is a(n) Question Blank 2 of 5 , pOH= 13.67 is a(n) Question Blank 3 of 5 , pOH= 7.00 is a(n) Question Blank 4 of 5 , [H+]= 5.3 x 10^-3 is a(n) Question Blank 5 of 5