acids and bases

When a base reacts with an acid, the…

H+ ion from the acid reacts

HCL + NaOH —> NaCl + H2O

Ionic eq

2HCL + CaCO3 —> CaCl2 + CO2 + H2O

volume equation

conc x old vol/new vol

Bronsted Lowry Acids and bases

Acid is a proton donor

Base is a proton acceptor

Monoprotic acid and base

Acid - substance that donates one proton

Base - substance that accepts only one proton (monobasic)

With Diprotic its 2

Diprotic acid example

H2SO4

rearrange to find conc

[H+] = 10^-pH

Acid base pair

Theory that acid has donated a proton air would be able to accept a proton back and then be a base

what is water in terms of acids and bases

amphoteric (water can behave as an acid and a base)

Strong acid

Acids completely ionise in water - all of H+ ions are released

Weak acid

These acids ionise partially in water - only some of the H+ ions are released

Dilute

Less acid molecules in a given volume of solution or more solvent present

Concentrated

Lots of acid molecules for a given volume in a solution

Common bases

Metal oxide and hydroxides And NH3

What is pH

Power of hydrogen

Decreasing pH..

Increases H+ by a factor of 10

pH formula

pH = - log 10 [H+]

pH must be 2 d.p.

H2SO4 thing

Calculate the pH when 250cm3 of 0.3 mol dm3 H2So4 made up to 1000cm3 solution

G dm3 to mol dm3

Divide by Mr

calculate pH of 0.2 mol dm3 HCL

0.70

conc of HCL with pH 3.55

2.81 × 10^-4

Kw equation

[products]/[reactants]

[H+][OH-] / [H2O]

H2O constant at room temp so simplifies to [H+][OH-] IN PURE WATER

[H+]²

Kw equation rearrangement

1.0 x 10⁻¹⁴ mol² dm⁻⁶

pK and pKa

pK_a = -log₁₀K_a

K_a = 10^-pKa