Marissa Levy Boyi Zhang Shana Zucker

Arrhenius Acid- An acid is a substance that when dissolved increases H + concentration Base- A base is a substance that when dissolved increases OH - concentration Bronsted-Lowry Acid- An acid is a substance that donates a proton Base- A base is a substance that accepts a proton Lewis Acid- An acid is a substance that is an electron-pair acceptor Base- A base is a substance that is an electron-pair donor Brönsted - Lowry Arrhenius Lewis

What’s an acid and what is a base? NH 3 + H 2 0 ⇆ NH OH - Base Acid Conjugate Acid Conjugate Base

Strong 1.Disassociate 2.Ionize completely Weak 1.Disassociate 2.Ionize Partially 3.Have K a or K b values

How do you calculate pH of a strong solution at equilibrium? 1.Write the equilibrium equation 2.Whatever concentration you start with is the concentration you end with 3.Calculate the pH

How do you calculate pH of a strong solution at equilibrium? 0.25 M of HClO 3 in water. KOH(aq) + H 2 0 (l) ⇆ K + (aq) + OH - (aq).25 M M+.25 M 0.25 M pOH= -log(.25)=.602 pH= 14- pOH= 13.40

How do you calculate pH of a weak solution at equilibrium? 1.Write the equilibrium equation 2.Write the ICE equation 3.Solve for X 4.Calculate the pH

How do you calculate pH of a solution at equilibrium?’ A 0.25 M Phosphoric solution is prepared in water. K a = 7.5 x H 3 PO 4 + H ₂ O (l) ⇆ H + + H 2 PO 4 - K a = 7.5 x x = x 2 /.25 x= pH= -log(.0433)= M00 -x+x.25 -xxx

N 1 C 1 V 1 = N 2 C 2 V 2 If 15.0 mL of HCN is completely titrated with 25.0 mL of M NaOH calculate the concentration of HCN. 1(C 1 ) (15.0)= 1(.100)(25.0) C1=.167 M

Strong Acid Strong Base H + + OH - ⇆ H ₂O (l)

Weak Acid Strong Base H 3 PO 4 + OH - ⇆ H ₂ O (l) + H 2 PO 4 - Weak Acid Weak Base HF + N 2 H 4 ⇆ HN 2 H F -

Buffer 1.A weak-acid base conjugate pair 2.They resist changes in pH

pH= pK a + log (base)/(acid) pOH= pK b + log (acid)/(base)

Sources  1/ss/titrationcurves_2.htm 1/ss/titrationcurves_2.htm  LabTutorials/Buffer/Buffer.html LabTutorials/Buffer/Buffer.html  2/ 2/