Question

The reaction of the strong acid HBr with the strong base KOH is: HBr(aq) + KOH(aq)...

The reaction of the strong acid HBr with the strong base KOH is: HBr(aq) + KOH(aq) -->HOH(l)+KBr(aq).Compute the pH of the resulting solution if 6.0 × 101mL of 0.55M acid is mixed with 31mL of 0.42M base. Let\'s do this in steps: How many moles of acid before reaction? How many moles of base before reaction? What is the limiting reactant? How many moles of the excess reagent after reaction? What is the concentration of the excess reagent after reaction? What is the pH of the resulting solution?

Show all the work. Thank you.

  

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
the reaction of the strong acid HBr with the strong base KOH is: HCl(aq) + CH3NH2(aq)...
the reaction of the strong acid HBr with the strong base KOH is: HCl(aq) + CH3NH2(aq) --> CH3NH+2 (aq) + Cl-(aq) To compute the pH of the resulting solution if 39mL of 0.45M acid is mixed with 51mL of 0.76M base. Let's do the stoich steps: How many moles of acid? How many moles of base? What is the limiting reactant? How many moles of the excess reagent after reaction? What is the concentration of the excess reagent after reaction?...
the reaction of the strong acid HCN with the strong base KOH is: HCN(aq) + KOH(aq)...
the reaction of the strong acid HCN with the strong base KOH is: HCN(aq) + KOH(aq) --> HOH(l) + KCN(aq) To compute the pH of the resulting solution if 63mL of 0.67M HCN is mixed with 26mL of 0.41M KOH. Let's do this in using stoich steps: How many moles of acid? How many moles of base? What is the limiting reactant? How many moles of the excess reactant after reaction? What is the concentration of the excess reactant after...
For all of the following questions 20.00 mL of 0.192 M HBr is titrated with 0.200...
For all of the following questions 20.00 mL of 0.192 M HBr is titrated with 0.200 M KOH. Region 1: Initial pH: Before any titrant is added to our starting material What is the concentration of H+ at this point in the titration? M What is the pH based on this H+ ion concentration? Region 2: Before the Equivalence Point 10.13 mL of the 0.200 M KOH has been added to the starting material. Complete the BCA table below at...
consider a strong acid - strong base titration OF 35.00 mL sample of 0.175 m HBr...
consider a strong acid - strong base titration OF 35.00 mL sample of 0.175 m HBr with 0.200 m KOH what is the ph of a solution after 10.00 ml of the KOH has been added? Stichiometry only, no equilibrium
In a titration of a strong base with a strong acid 10mL of a .5M KOH...
In a titration of a strong base with a strong acid 10mL of a .5M KOH were added to a 25mL of a .25M HCl solution. Calculate the pH of the solution after the addition of the KOH.
Part D Enter a chemical equation for HBr(aq)HBr(aq)showing how it is an acid or a base...
Part D Enter a chemical equation for HBr(aq)HBr(aq)showing how it is an acid or a base according to the Arrhenius definition. Consider that strong acids and bases dissociate completely.
33 . Strong base is dissolved in 565 L of 0.600 M weak acid (?a=3.30×10−5 M)(Ka=3.30×10−5...
33 . Strong base is dissolved in 565 L of 0.600 M weak acid (?a=3.30×10−5 M)(Ka=3.30×10−5 M) to make a buffer with a pH of 4.08. Assume that the volume remains constant when the base is added. HA(aq)+OH−(aq)⟶H2O(l)+A−(aq) Calculate the pKa value of the acid and determine the number of moles of acid initially present. When the reaction is complete, what is the concentration ratio of conjugate base to acid? How many moles of strong base were initially added?
Strong base is dissolved in 645 mL of 0.400 M weak acid (Ka = 4.91 ×...
Strong base is dissolved in 645 mL of 0.400 M weak acid (Ka = 4.91 × 10-5) to make a buffer with a pH of 4.11. Assume that the volume remains constant when the base is added. Calculate the pKa value of the acid and determine the number of moles of acid initially present. When the reaction is complete, what is the concentration ratio of conjugate base to acid? How many moles of strong base were initially added?
Strong base is dissolved in 545 mL of 0.200 M weak acid (Ka = 4.02 ×...
Strong base is dissolved in 545 mL of 0.200 M weak acid (Ka = 4.02 × 10-5) to make a buffer with a pH of 4.11. Assume that the volume remains constant when the base is added. a) Calculate the pKa value of the acid and determine the number of moles of acid initially present. b) When the reaction is complete, what is the concentration ratio of conjugate base to acid? c) How many moles of strong base were initially...
10g (0.082 moles) of benzoic acid. 25mL (0.62 moles) of methanol. What is the limiting reagent...
10g (0.082 moles) of benzoic acid. 25mL (0.62 moles) of methanol. What is the limiting reagent in this reaction? Show how you arrived at this conclusion. Why do you think this reagent rather than the other was made limiting? How many fold excess is the reactant that is used in excess?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT