Question

what is the pH of an aqueous solution at 25 degrees celcius that is 3.3 m HNO3

Answer #1

**Answer** – Given, molality of HNO_{3} =
3.3 m

We know, molality means moles / kg of solvent

So, mass of solvent = 1 kg and we know density of water = 1.0 g/mL

So, volume of water = 1 kg = 1000 g = 1000 mL = 1 L

So, molarity of HNO_{3} = 3.3 M

We know HNO_{3} is strong acid

[HNO_{3}] = [H_{3}O^{+}] = 3.3 M

So, **pH** = -log [H_{3}O^{+}]

= - log 3.3 M

= **-0.52**

At 25 degrees Celcius, the density of a 30% aqueous solution by
weight of glycerol (C6H8O3) is
1.071 g/mL. What is the concentration of glycerol in this solution
in units of molarity, molality, and mole fraction?

An aqueous solution at 25 degrees celsius is 12.0% HNO3 by mass
and has a density of 1.055 g/mL. What is the pH?

An aqueous solution at 25 degrees celsius is 12.0% HNO3 by mass
and has a density of 1.055 g/mL. What is the pH?

For the aqueous [AlF6]3- complex
Kf= 4.0 x 1019 at 25 degrees celcius.
Suppose equal volumes of 0.0064 M Al
(NO3)3 solution and 0.50 M KF solution are
mixed. Calculate the equilibrium molarity of aqueous
Al3+ ion.
Round your answer to 2 signifcant digits.

What is the pH of a 0.25 M aqueous solution of KCHO2 at
25°C?
The Ka of HCHO2 is1.8 x 10-4 at 25°C.

What is the pH of a 0.108 M aqueous solution of
potassium acetate,
KCH3COO at 25 °C?
(Ka for CH3COOH =
1.8×10-5)

Calculate the pH at 25 degrees C of 211 mL of a buffer solution
that is 0.230 M NH4Cl and 0.230 M NH3 before and after the addition
of 1.6 mL of 6.0 M HNO3. The pKa for NH4+ is 9.75.

What is the pH of a 0.5 m solution of sodium propionate,
NaC3H5O2 at 25 degrees C?
(For propionic acid, HC3H5O2,
Ka = 1.3 x 10-5 at 25 degrees C)

Calculate the pH of each aqueous solution:
(a) 0.041 M HNO3;
(b) 0.0041 M NaOH

There are four aqueous solutions at 25 degrees celsius.
Solution A
Given [H+] = 1.3 x 10-9 M, find
[OH-], pH, and pOH.
Solution B
Given [OH-] = 0.098 M, find [H+], pH, and
pOH.
Solution C
Given pH = 8.16, find [H+], [OH-], and
pOH.
Solution D
Given pOH = 1.03, find [H+], [OH-], and
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