Unit 13 Marker Board Review. Acids & Bases Made with love and care by. Question #1. List 4 properties of acids. Answer: 1 – Sour taste 2 – React with metals to form hydrogen gas 3 – React with metal carbonates to form CO 2 gas 4 – Turn indicators red. Question #2.
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Unit 13 Marker Board Review
Acids & Bases
Made with love and care by
List 4 properties of acids.
1 – Sour taste
2 – React with metals to form hydrogen gas
3 – React with metal carbonates to form CO2 gas
4 – Turn indicators red
List 4 properties of bases.
1 – Taste bitter
2 – Unreactive with metals and carbonates
3 – Feel slippery
4 – Turn indicator blue
According to Arrhenius, acids must contain _______ ions & bases must contain _______ ions.
A Bronsted acid _____________ a _______________ and a base ______________ a ____________.
- hydrogen ion
- hydrogen ion
Label the Acid, Base, Conj Acid, Conj Base
NH3 + H2O NH4+ + OH-
B A CA CB
H2CO3 + H2O H3O+ + HCO3-
A B CA CB
Base anhydrides contain a _________________ and oxygen.
Acid anhydrides contain a _________________ and oxygen.
When an acid reacts with a base to neutralize it, the products are a _______________ & ___________.
Answer: Salt & Water
Pure water has a pH of _________ because …
Answer: 7…Because it is neutral!
Acids have a pH ___________ than 7; bases _____________ than 7.
Write the name for the following formulas. Is it an acid or base?
Check your answers after you’ve written ALL of them!
Hydrocyanic Acid - acid
Magnesium Hydroxide - base
Write & balance the equation for the neutralization of sulfuric acid with potassium hydroxide.
Answer: H2SO4 + 2 KOH 2 H2O + K2SO4
Write & balance the neutralization reaction of hydrobromic acid & calcium hydroxide.
2 HBr + Ca(OH)2 2 H2O + CaBr2
The formula for the hydronium ion is ____________________ & for the hydroxide ion _______________.
Answer: H30+& OH-
An H+ ion is really just a _______________ and cannot exist in solution.
Write the equation for the self-ionization of water.
Answer: H2O + H2O OH- + H3O+
The formula for calculating [H3O+] from pH is ______________________. I type this into my calculator as: _________
Answer: [H3O+] = 10^(-pH)
2nd log (negative pH)
The formula for calculating [H3O+] from [OH-] is ______________________. I type this into my calculator as: _______
Answer: Kw = [OH-][H3O+] = 1.0 x 10-14
[H3O+] = 1.0 x 10-14
1.0 E -14 / [OH-]
pH = -log [H+] OR 14 - pOH
[H+] = 10^(- pH) OR 1.0 x 10-14 / [OH-]
pOH = -log [OH-] OR 14 - pH
[OH-] = 10^(- pOH) OR 1.0 x 10-14 / [H3O+]
What is the pH of an HCl solution with a concentration of 0.0015 M?
Answer: pH = 14 – pOH = 14 – 10.5 = 3.5
Answer: [H+] = 10^(-4.51) = 3.09 x 10-5 M
Answer: pOH = -log [OH-]
[OH-] = 1.0 x 10-14 / 9.99 x 10-9 = 1.0 x 10-6 M
pOH = -log(1.0 x 10-6) = 6.0
Answer: pOH = -log [OH-] = -log (7.81x10-3) = 2.1
Answer: [OH-] = 10^(-5.21) = 6.17 x 10-6 M.
What is the purpose of a titration? What is the role of an indicator in a titration?
Answer: A titration enables you to determine the concentration of a solution by reacting a known volume of the solution with a solution of known concentration.
An indicator changes color when the end point of the titration has been reached.
Answer: The concentration of H3O+ has decreased. The substance is a base.