Question

Sulfuric acid is a strong acid and dissociates in water as shown in Equation 5. H2SO4...

Sulfuric acid is a strong acid and dissociates in water as shown in Equation 5.

H2SO4 (aq) = 2H+ (aq) + SO42− (aq)     (Equation 5)

What is the hydrogen ion concentration, in mol dm−3 when 2.00 g of sulfuric acid is dissolved in water to give 0.400 dm3 of solution? (Show all of your working and give your answer to three significant figures.)

What is the corresponding pH of the solution in part (b)(i)? (Show all of your working and give your answer to two significant figures.)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid....
To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid. Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as H2SO4?H++HSO4? A HSO4? anion can dissociate further by HSO4??H++SO42? but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as Ka2=[H+][SO42?][HSO4?]=0.012 Part A Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid....
To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid....
To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid. Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as H2SO4?H++HSO4? A HSO4? anion can dissociate further by HSO4??H++SO42? but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as Ka2=[H+][SO42?][HSO4?]=0.012 Part A Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid....
± The Nernst Equation and pH Sulfuric acid is a very strong acid that can act...
± The Nernst Equation and pH Sulfuric acid is a very strong acid that can act as an oxidizing agent at high concentrations (very low pH, or even negative pH values). Under standard conditions, sulfuric acid has a low reduction potential, SO42−(aq)+4H+(aq)+2e−⇌SO2(g)+2H2O(l),   +0.20 V which means it cannot oxidize any of the halides F2, Cl2, Br2, or I2. If the H+ ion concentration is increased, however, the driving force for the sulfuric acid reduction is also increased according to Le Châtelier's...
1) sulfuric acid reacts with the ammonia according to the equation below. It takes 32.89 mL...
1) sulfuric acid reacts with the ammonia according to the equation below. It takes 32.89 mL of a 1.50 M solution of sulfuric acid to neutralize 64.7 mL of ammonia solution. what is the molar concentrationof the ammonia solution? H2SO4 (aq) + 2 NH3 (aq)---> (NH4)2SO4 (aq) 2) A 500.0mL solution that contains silver ion is treated with excess sodium chloride soultion, producing a precpitate of silver chloride that has a mass of 45.4 mg. What mass of silver ion...
1) a. Write the balanced molecular equation that occurs for the complete reaction of sulfuric acid...
1) a. Write the balanced molecular equation that occurs for the complete reaction of sulfuric acid with sodium hydroxide. b. To determine the molarity of your final sulfuric acid solution, you titrate the final solution with a standardized sodium hydroxide solution to the second equivalence point. If 26.32 mL of 0.1000 M sodium hydroxide was required for complete reaction with 10.00 mL of the final sulfuric acid solution, determine the molarity of the final sulfuric acid solution precisely to four...
Sulfuric acid is a very strong acid that can act as an oxidizing agent at high...
Sulfuric acid is a very strong acid that can act as an oxidizing agent at high concentrations (very low pH, or even negative pH values). Under standard conditions, sulfuric acid has a low reduction potential, SO42−(aq)+4H+(aq)+2e−⇌SO2(g)+2H2O(l),   +0.20 V which means it cannot oxidize any of the halides F2, Cl2, Br2, or I2. If the H+ ion concentration is increased, however, the driving force for the sulfuric acid reduction is also increased according to Le Châtelier's principle. Sulfuric acid cannot oxidize the...
A volume of 60.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution...
A volume of 60.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 11.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) Express your answer with the appropriate units. Hints Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution...
1. An aqueous solution of sulfuric acid (6M H2SO4 in water) is flowing into a tank...
1. An aqueous solution of sulfuric acid (6M H2SO4 in water) is flowing into a tank at the rate of 100 liters/min (also can be written 100 L/min) having a density of 1.34 g/cm3. Calculate value of the items requested below and make sure you show HOW you obtained them. For parts (b) - (d), first write out the equation using symbols for the appropriate variables, and then algebraically solve for the unknown variables, and finally substitute in the numerical...
Based off info below please answer blank boxes. Thanks! Application Questions: 12. Before using a solution...
Based off info below please answer blank boxes. Thanks! Application Questions: 12. Before using a solution of NaOH as a standard for a titration, its precise concentration must be determined by titration with a standard acid. This is because solid NaOH absorbs water from the atmosphere, so its solid form is difficult to keep free of contaminated H2O. A common acid used for standardization is the acid-salt, potassium hydrogen phthalate (KHP), KHC8H4O4. Another way is to use a standardized solution...
Q. When a pink aqueous solution of potassium permanganate, faintly acidified with dilute sulfuric acid was...
Q. When a pink aqueous solution of potassium permanganate, faintly acidified with dilute sulfuric acid was treated with 10% aq. hydrogen peroxide, the reaction took place with the evolution of gas bubbles, and the pink solution was turned colorless. Further chemical analysis revealed that the evolved gas was oxygen, and the resulting solution contains potassium sulfate and manganese (II) sulfate; water was also formed during the same reaction. Please answer the followings: 1) Write down the balanced chemical equation for...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT