Question

A 5.00-mL sample of nitric acid required 13.25 mL of 0.0842 M strontium hydroxide for titration....

A 5.00-mL sample of nitric acid required 13.25 mL of 0.0842 M strontium hydroxide for titration. Calculate the molarity of the acid solution. (Hint: It's stoichiometry, you need the balanced equation)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The balanced chemical equation is as shown.


One mole of strontium hydroxide reacts with 2 moles of nitric acid.
Number of moles of strontium hydroxide moles
Number of moles of nitric acid moles.
Molarity of nitric acid

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
35.00 mL of unknown calcium hydroxide solution is titrated with 0.250 M standard nitric acid solution....
35.00 mL of unknown calcium hydroxide solution is titrated with 0.250 M standard nitric acid solution. if 40.09 mL of the standard acid solution is required to reach a phenolphthalein endpoint, what is the molarity of the unknown calcium hydroxide solution? write the balanced formula unit equation.
a) A strontium hydroxide solution is prepared by dissolving 10.55 g of Sr(OH)2 in water to...
a) A strontium hydroxide solution is prepared by dissolving 10.55 g of Sr(OH)2 in water to make 59.00 mL of solution.What is the molarity of this solution? (1.470M is the right answer) b) Next the strontium hydroxide solution prepared in part (a) is used to titrate a nitric acid solution of unknown concentration.Write a balanced chemical equation to represent the reaction between strontium hydroxide and nitric acid solutions. c) If 23.9 mL of the strontium hydroxide solution was needed to...
A strontium hydroxide solution is prepared by dissolving 10.40 g of Sr(OH)2 in water to make...
A strontium hydroxide solution is prepared by dissolving 10.40 g of Sr(OH)2 in water to make 47.00 mL of solution.What is the molarity of this solution? Express your answer to four significant figures and include the appropriate units. SubmitMy AnswersGive Up Part B Next the strontium hydroxide solution prepared in part (a) is used to titrate a nitric acid solution of unknown concentration.Write a balanced chemical equation to represent the reaction between strontium hydroxide and nitric acid solutions. Express your...
Test your understanding of titrations. Write a balanced equation for the neutralization of aqueous strontium hydroxide...
Test your understanding of titrations. Write a balanced equation for the neutralization of aqueous strontium hydroxide with aqueous hydrochloric acid. A chemist finds a strontium hydroxide solution in lab, but the concentration of this solution is not labeled. A 25.00 mL sample of strontium hydroxide solution is placed in a flask. It takes the addition of 30.00 mL of 0.2695 M HCl to reach the equivalence point. What is the molarity of the strontium hydroxide solution? [0.1617 M] What is...
The molarity of an aqueous solution of potassium hydroxide ( KOH ) is determined by titration...
The molarity of an aqueous solution of potassium hydroxide ( KOH ) is determined by titration against a 0.171 M nitric acid ( HNO3 ) solution. If 25.0 mL of the base are required to neutralize 10.4 mL of nitric acid , what is the molarity of the potassium hydroxide solution?
Answer question 9a and 9b using the reaction equation between nitric acid reacts with magnesium hydroxide....
Answer question 9a and 9b using the reaction equation between nitric acid reacts with magnesium hydroxide. 2 HNO3(aq) + Mg(OH)2(aq) →Mg(NO3)2(aq) + 2 H2O (aq) 9a. A 35.00 mL of sample of nitric acid solution is required to neutralized 20.0 mL of 0.550 M magnesium hydroxide solution. Calculate the molarity of the nitric acid solution. 9b. If 50.0 mL of 0.250 M nitric acid solution is reacted with 25.0 mL of 0.550 M of magnesium hydroxide solution, then many molecules...
The molarity of an aqueous solution of sodium hydroxide ( NaOH ) is determined by titration...
The molarity of an aqueous solution of sodium hydroxide ( NaOH ) is determined by titration against a 0.132 M nitric acid ( HNO3 ) solution. If 31.9 mL of the base are required to neutralize 29.2 mL of nitric acid , what is the molarity of the sodium hydroxide solution? Give your answer to three significant figures.
In a titration of 44.16 mL of 0.3336 M nitric acid with 0.4575 M aqueous sodium...
In a titration of 44.16 mL of 0.3336 M nitric acid with 0.4575 M aqueous sodium hydroxide, what is the pH of the solution when 44.16 mL of the base have been added? Please go by steps! Thank you!
43.       In a titration of 35.35 mL of 0.3509 M nitric acid with 0.4242 M aqueous...
43.       In a titration of 35.35 mL of 0.3509 M nitric acid with 0.4242 M aqueous sodium hydroxide, what is the pH of the solution when 35.35 mL of the base have been added?
A. A 11.3 g sample of an aqueous solution of hydrobromic acid contains an unknown amount...
A. A 11.3 g sample of an aqueous solution of hydrobromic acid contains an unknown amount of the acid. If 12.8 mL of 0.122 M barium hydroxide are required to neutralize the hydrobromic acid, what is the percent by mass ofhydrobromic acid in the mixture? = % by mass B. A 10.4 g sample of an aqueous solution of nitric acid contains an unknown amount of the acid. If 25.9 mL of 0.403 M barium hydroxide are required to neutralize...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT