the
concentration of hydronium ions C in a solution with a pH of x is C...
the
concentration of hydronium ions C in a solution with a pH of x is C
= 10^-x, with C measured in moles per liter. How quickly is the pH
changing when the pH is 9 and the concentration is increasing by
2(10^-10) (moles per liter) per minute?
Solutions
Expert Solution
Using the chain rule, we will differentiate the concentration
function C(x) with respect to 't', we get dx/dt using the given
condition, dC/dt= 2(10-10) when x=9.
5. The concentration of hydronium ions C in a solution with a pH
of x is C = 10−x , with C measured in moles per liter. How quickly
is the pH changing when the pH is 9 and the concentration is
increasing by 2 · 10−10 (moles per liter) per minute?
6. A spherical balloon is being deflated while keeping its
shape. How quickly is its surface area changing when the radius is
3 cm and the volume is...
Calculate the concentration of hydronium ions in: (a) a solution
that is 0.20M HBrO(aq) and 0.10M KBrO(aq); (b) a solution that is
0.010M (CH3)2NH(aq) and 0.150M
(CH3)2NH2Cl(aq); (c) a solution
that is 0.10M HBrO(aq) and 0.20M KBrO(aq); (d) a solution that is
0.020M (CH3)2NH(aq) and 0.030M
(CH3)2NH2Cl(aq).
The hydronium ion concentration of a pH neutral
aqueous solution is decreased by three orders of magnitude.
Is it acidic or basic?
pH increase or decrease?
By how many pH units does the pH change?
Does the molar concentration of hydroxide increase or
decrease?
By how many orders of magnitude does the molar concentration of
hydroxide change?
1. Calculate the hydronium ion concentration and pH for a 0.042
M solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion
with water is 5.6 × 10-11.
[H3O+]----------------M
pH---------------------
2.
What are the equilibrium concentrations of NH3,
NH4+, and OH- in a 0.42 M solution
of ammonia? What is the pH of the solution?
Kb = 1.8 * 10^-5
[OH-] ----------------------- M
[NH4+] ----------------------M
[NH3] ---------------------- M
pH----------------------------
Calculate the hydronium ion concentration and pH for a 0.050 M
solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion
with water is 5.6 × 10-11.
[H3O+] =_____ M
pH =______
Solid aluminum is added to a solution of sulfuric acid and
hydronium (hydrated hydrogen) ions, forming a solution that
consists of aluminum(III) ion, liquid water, and solid sulfur.
(a) Using a table of standard reduction
potentials, write the half-reaction equations for each of the redox
reactions indicated.
(b) Modify the half-reactions, if
necessary, and add them to yield a balanced net ionic equation.
(c) Calculate E° for the reaction as
written.
(d) State and justify the favored
direction of the reaction.
Calculate the hydronium ion concentration and the pH when 65.0
mL of 0.45 M NH3 is mixed with 65.0 mL of 0.45 M HCl (Ka =
5.6x10^-10).
Concentration =
pH=