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Titration
Terms
Equations
Buffers
Indicators
100
This is titrated to a weak acid to give an equivalance point pH less than 7.
What is a strong base?
100
This is an ion that decreases the pH of a solution but does not fully dissociate.
What is a weak acid?
100
This is the net ionic equation for NH4+ and NaOH.
OH- + NH4+ --> NH3 + H2O ?
100
You would add this to a solution of ammonia to make it a buffer.
What is ammonium?
100
Bromocresol purple turns this color in a basic solution.
What is purple.
200
This amount of 5M H2SO4 is needed to fully titrate 1.000L of 1M NaOH.
What is .100L?
200
This term that is used to describe an ion that is able to donate a hydrogen cation.
What is a Bronsted-Lowry acid?
200
This is the net ionic equation for ammonia and sodium bicarbonate.
NH3 + HCO3- --> NH4+ + CO3-2 ?
200
This base would be used to form a buffer with HBr.
What is Br-?
200
Phenolphthalein turns this color in a basic solution.
What is pink.
300
Phenophthalein (color changes at 8.2-12.0) is used to indicate a titration between these two.
What is a strong base/weak acid?
300
This is the mother of all weak bases.
What is ammonia(NH3)?
300
This is the net ionic equation between hydrochloric acid and potassium bicarbonate.
What is H+ + KHCO3 --> H2O + CO2 + K+ ?
300
Phenophthalein turns this color in an acidic solution.
What is colorless.
400
Phenol red(color changes at pH of 6.4-8.0) in calcium hydroxide would be best titrated with this.
What is any stong acid?
400
This is a Lewis Base.
What is an ion that donates a lone pair of electrons?
400
This is the balanced equation for amine.
What is 2NH2- + 2H2O--> 2NH3 + 2OH-
400
This is the pH of 50.00 mL buffer solution which is 2.00M in HCl2H3O2 and 2M in NaC2H3O2. Ka of acetic acid=1.8x10-5.
What is 4.74? 
pH = -log(1.85×10-5) + log(2.00 / 2.00)
pH = -log(1.85×10-5) + 0
pH = 4.74
400
This ion has a higher concentration when litmus is red.
What is H3O+ or H+.
500
Titration reveals that 11.6mL of 3.0M H2SO4 is required to neutralize a 25.0mL solution of NaOH showing this is the molarity of the NaOH solution.
What is 2.8 M?
500
This is the difference between amphiprotic and ampiteric.
What is amphiprotic can donate and accept a proton while ampiteric can act either as a base or an acid?
500
Write the balanced equation for NaNH2 + Zn(NH2)2
2NaNH2 + Zn(NH2)2 --> Na2[Zn(NH2)4]
500
This is the pH for a solution of 1 mol ammonium and 1 mol ammonia when 36.5g of HCl is added . Ka of ammonium=5.9x10-10
What is 4.61? 

5.9×10-10 = x2/1
[H+] = 2.4x10-5
pH = -log(2.4×10-5)
pH = 4.61
500
This indicator would be used for titration with an equivilance point around 4.4 to 6.3.
What is methyl red?