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Titration
Terms
Equations
Buffers
Indicators
100
The equivalence point.
What is The point in a titration at which the reaction between titrant and unknown has just been completed.
100
This is an ion that decreases the pH of a solution but does not fully dissociate.
What is a weak acid?
100
pH=pKa + log([base]/[acid])
What is the Henderson–Hasselbalch equation?
100
This is what a buffer is made of.
What is a weak acid/base and its conjugate?
100
The purpose of indicators.
What is to determine when pH passes a given point?
200
This is titrated to a weak acid to give an equivalance point pH greater than 7.
What is a strong base?
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 NH4+ and NaOH.
What is OH- + NH4+ --> NH3 + H2O ?
200
You would add this to a solution of ammonia to make it a buffer.
What is ammonium?
200
Is what an indicator is usually made of.
What is is a weak acid?
300
This amount of 5M HCl is needed to fully titrate 1.000L of 1M NaOH.
What is 200ml?
300
This is a Lewis Base.
What is an ion that donates a lone pair of electrons?
300
This is the net ionic equation for NH3 and NaHCO3.
What is NH3 + HCO3- --> NH4+ + CO3-2 ?
300
This base would be used to form a buffer with HBr.
What is What is Br-?
300
The indicator used for used for determining when a solution has become acidic in particular pH 5.
What is methyl red?
400
Titration reveals that 12.5mL of 3.0M HCl is required to neutralize a 25.0mL solution of NaOH showing this is the molarity of the NaOH solution.
What is 1.5M
400
This is the net ionic equation between HCl acid and KHCO3.
What is What is H+ + KHCO3 --> H2O + CO2 + K+ ?
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 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
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
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 What is 4.61? 5.9×10-10 = x2/1 [H+] = 2.4x10-5 pH = -log(2.4×10-5) pH = 4.61