T6A

lecture ws

lecture ws

Reaction hwere one molecule trnasfers a proton to a proton to a molecule of the same kind

Autoprotolysis

Kw=

1.0x10⁻¹⁴

H₂O can act as both an acid or a base

Amphiprotic

Species formed when the base accepts a proton

Conjugate acid

Species formed when the acid donates a proton

Conjugate base

Complete this equation to show how pyridine, C₅H₅N,acts as a Bronsted-Lowry base in water HW 4.3

C₅H₅N + H₂O⇌ C₅H₆N⁺ + OH⁻

[H₃O⁺][OH⁻]=

Kw= 1.0x10⁻¹⁴

Rank from strongest acid to weakest acid: HClO₃ HClO HClO₄ HClO₂ HW 4.8

Strongest HClO₄ HClO₃ HClO₂ HClO Weakest

Estimate the concentrations of a) H₃O⁺ b) OH⁻ at 25°C in 2.2x10⁻³M NaOH(aq) Self Test 6A.3B

a) 4.5x10⁻¹² b) 2.2x10⁻³

Write the formula for the conjugate acids of a) CH₃NH₂ b) NH₂NH₂ c)HCO⁻₃ Write the formula for the conjugate bases of d)HCO⁻₃ e)C₆H₅OH f)CH₃COOH Exercise 1

a) CH₃NH₃⁺ b) NH₂NH₃⁺ c) H₂CO₃ d) CO₃²⁺ e)C₆H₅O⁻ f) CH₃COO

What is a) the conjugate acid of OH⁻ b) the conjugate base of HPO₄⁻² Self Test 6A.1A

a) H₂O b) PO³⁻₄

a)Solution A: -Given: [H⁺]= 3.3x10⁻¹¹ -Find: [OH⁻] pH pOH b) Solution B: -Given: [OH⁻]= 6.4x10⁻¹² -Find: [H⁺] pH pOH c) Solution C: -Given: pH= 7.31 -Find: [H⁺] [OH⁻] pOH d) Solution D: -Given pOH= 2.68 -Find: [H⁺] [OH⁻] pH HW 4.4

a) Solution A: [OH⁻]= 3.0x10⁻⁴ pH= 10.48 pOH= 3.52 b) Solution B: [H⁺]= 1.56x10⁻³ pH= 2.81 pOH= 11.19 c) Solution C: [H⁺]= 4.9x10⁻⁸ [OH⁻]= 2.04x10⁻⁷ pOH= 6.69 d) Solution D: [H⁺]= 4.79x10⁻¹² [OH⁻]= 2.09x10⁻³ pH= 11.32

Calculate the molar concentration of OH⁻ in solutions with the following molar concentrations of H₃O⁺ a) .020 M b) 1.0x10⁻⁵ M c) 3.1 M Exercise 19

a)5.0x10⁻¹³ b)1.0x10⁻⁹ c)3.2x10⁻¹⁵

Give the conjugate base for each compound below acids: a) H₂SO₄ b) H₄PO₄⁻ c) NH₄⁺ HW 4.1

a)HSO⁻₄ b)HPO⁻²₄ c)NH₃

What is a) the conjugate acid of H₂O b) the conjugate base of NH₃ Self Test 6A.1B

a)H₃O⁺ b)NH⁻₂

Give the conjugate acid for each compound below Base: a)H₂PO⁻₄ b)S²⁻ c)NH₃ HW 4.2

a)H₃PO₄ b)HS⁻ c)NH⁺₄

Classify these compounds as Strong acids, weak acids, Strong bases, weak bases or other a)CH₃COOH b) NaCl c) HNO₃ d)NaOH e) (CH₃)₃N f)HNO₃ g)H₂CO₃ h)HCN i)Ba(OH)₂ j)NH₃ HW 4.5

a)weak acid b)other c)Strong acid d)Strong base e)Weak base f)Strong acid g)Weak acid h)Weak acid i) Strong base j) Weak base

What is the pH of a 2.9 M solution of HClO₄? HW 4.7

pH= -0.46