Acids, Bases, and Nuclear Chemistry Flashcards

Flashcards for acids, bases, pH, and nuclear chemistry

Strong Acids

Sulfuric acid, nitric acid, hydrochloric acid, and hydrobromic acid

Brønsted-Lowry Base Example

NH3 (Ammonia)

Neutralization Reaction Consequence

Water formation

Conjugate Base of CH3COOH

CH3COO–

Acidic pH

pH < 7 (e.g., 2)

pH Calculation [H+] = 10–2 M

pH = 2

pH Calculation [H+] = 2.5 × 10–5 M

pH = -log(2.5 x 10^-5)

pH + pOH

Sum of pH and pOH = 14

Increasing Basicity of Conjugate Bases

CN– < CH3COO– < NO2 – (from HNO2 > CH3COOH > HCN)

Buffer Properties

Resists changes in pH; weak acid and its conjugate base

[H+] in 0.5 M H2SO4

1 M

Acid Rain Formation

Sulfur dioxide and NOx emissions

Volume of 0.30 M NaOH to Neutralize 50 mL of 0.75 M HCl

125 mL

Amphoteric Substance

H2PO4 –

Neutrons in € 19 F

10

Protons in 20 42Ca 2 +

20

Neutrons in € 133Xe

79

Remaining 131I After 32 Days

7.5 g (initial 120g, half-life 8 days)

X in Nuclear Reaction 1 2 H+ 1 3 H→2 3 He + X

2 neutrons

Decay of 214Bi with Alpha Emission

81 210Tl

Rn (222) Decay

82 214Pb

Increasing Energy of Electromagnetic Radiation

microwaves < red light < yellow light < gamma rays

Isotope of 92 235 U

92 238 U

Proton Converted into Neutron Emission

Positron

Transmutation

Conversion of one element to another