5. The concentration of hydronium ions C in a solution with a pH of x is...

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 decreasing by 1 cubic centimeter per second? (Hint: first find out how quickly the radius is changing.)

Expert Solution

milcah answered 2 years ago

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?

Calculate the concentration of hydronium ions in: (a) a solution that is 0.20M HBrO(aq) and 0.10M...

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).

What is the concentration of hydronium ions after a 100mL solution of 0.02M Magnesium Hydroxide and...

What is the concentration of hydronium ions after a 100mL solution of 0.02M Magnesium Hydroxide and 100mL of 0.05M nitric acid?

The hydronium ion concentration of a pH neutral aqueous solution is decreased by three orders of...

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,...

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....

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 =______

Calculate the hydronium ion concentration and the pH when 50.0ml of 0.40M NH3 is mixed with...

Calculate the hydronium ion concentration and the pH when 50.0ml of 0.40M NH3 is mixed with 50.0ml of 0.40M Hcl

Solid aluminum is added to a solution of sulfuric acid and hydronium (hydrated hydrogen) ions, forming...

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...

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=

The hydronium ion concentration of an aqueous solution of 0.530 M hydroxylamine (a weak base with...

The hydronium ion concentration of an aqueous solution of 0.530 M hydroxylamine (a weak base with the formula NH2OH) is ... [H3O+] = ____M

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