How much does the pH of 20.0 mL of a 0.75 M ammonium chloride
(NH4Cl) solution change upon the addition of 15.0 mL of 1.0 M NaOH?
Ka for ammonia (NH4+) 5.69 x 10-10?
1. In one step, ammonium chloride (NH4Cl) was added to lower the
blood pH. The ammonium ion is what acts as the acid. The chloride
ion does not have any acid/base properties.
a. Why is the ammonium ion used as the acid source instead of
HCl?
b. Why is NH4Cl used instead of some other ammonium compound
(such as NH4NO3 or NH4I)?
Activity 4: Equilibrium of solid ammonium chloride with ammonium
chloride in aqueous solution. NH4Cl(s) +H2O(l) NH4+(aq) + Cl-(aq)
(ammonium chloride) (ammonium ion) Procedure * Pour about 75 mL of
tap water into a 150-mL beaker and heat to boiling on a hot plate.
* While waiting for the water to boil, place approx. 1 mL of a
saturated NH4Cl solution into a small, clean, dry test tube. *To
this test tube, add concentrated HCl solution one drop at a...
a) A buffer contains significant amounts of both ammonia (NH3)
and ammonium chloride (NH4Cl). Write the net ionic equation showing
how this buffer neutralizes added HI. Express your answer as a
chemical equation.
b)A buffer contains significant amounts of both ammonia (NH3)
and ammonium chloride (NH4Cl). Write the net ionic equation showing
how this buffer neutralizes added NaOH. Express your answer as a
chemical equation.
In a particular solution, acetic acid is 11% ionized at 25°C.
Calculate the pH of the solution and the mass of acetic acid
(Ka=1.8x10^-5) dissolved to yield 1.00 L of solution.
pH = __
Mass = __ g
Solid ammonium chloride, NH4Cl, is formed by the reaction of
gaseous ammonia, NH3, and hydrogen chloride,
HCl.NH3(g)+HCl(g)⟶NH4Cl(s)
A 6.37 g sample of NH3 gas and a 6.37 g sample of HCl gas are
mixed in a 1.00 L flask at 25 ∘C.
How many grams of NH4Cl will be formed by this reaction?
What is the pressure in atmospheres of the gas remaining in the
flask? Ignore the volume of solid NH4Cl produced by the
reaction.
What is the pH of a 100 mL solution of 100 mM acetic acid at pH
3.2 following addition of 5 mL of 1 M NaOH? The pKa of acetic acid
is 4.70.
A) 3.20.
B) 4.65.
C) 4.70.
D) 4.75.
E) 9.60.
a solution of acetic acid on a labratory shelf was of
undetermined concentration. if the PH of the solution was found to
be 2.57 what was the concentration of the acetic acid. The Ka of
the Acidic acid is 1.7x10^-5