0.400 L of HBr were neutralized with 0. 2 L of a 6 M KOH solution....

Question

Question

0.400 L of HBr were neutralized with 0. 2 L of a 6 M KOH solution. What was the molarity of the acid neutralized?

science chemistry

Answer 1

Answer #1

The balanced equation is

KOH + HBr ------> KBr + H₂O

Number of moles of KOH = molarity * volume of solution in L

Number of moles of KOH = 6 * 0.2 = 1.2 mole

From the balanced equation we can say that

1 mole of KOH requires 1 mole of HBr so

1.2 mole of KOH will require

= 1.2 mole of KOH *(1 mole of HBr / 1 mole of KOH)

= 1.2 mole of HBr

Molarity of HBr = number of moles of HBr / volume of solution in L

Molarity of HBr = 1.2 / 0.400 = 3 M

Therefore, the molarity of acid = 3 M

Answer 2

Similar Homework Help Questions

A 10.0mL of 0.121 M H2SO4 is neutralized by 17.1 mL of KOH solution according to the following balanced chemical reactio...

A 10.0mL of 0.121 M H2SO4 is neutralized by 17.1 mL of KOH solution according to the following balanced chemical reaction. H2SO4(aq) + 2 KOH(aq)-----> K2SO4(aq) + 2 H2O(l) A) Find the number of moles of KOH that neutralized 10.0mL of 0.121 M H2SO4. B) What is the molarity of the KOH solution?
9. a If 25.0 mL of KOH solution is neutralized by 13.31 mL of 0.111 M...

9. a If 25.0 mL of KOH solution is neutralized by 13.31 mL of 0.111 M H3PO4, what is the molarity of the KOH? State formula, of course you were going to do that, right? b) How many mL of 0.123 M H2SO4 solution is needed to neutralize 25,0 mL of 0.250 M KOH solution?
what is the molarity of a KOH solution if 25.0 ml of it is neutralized by...

what is the molarity of a KOH solution if 25.0 ml of it is neutralized by 31.7 ml of 0.100M nitric acid solution?

An aqueous solution of 0.100 M phosphoric acid (12.0 mL) is titrated with 0.400 M KOH...

An aqueous solution of 0.100 M phosphoric acid (12.0 mL) is titrated with 0.400 M KOH as shown below. phosphoric acid has three pKas: 2.148, 7.198, 12.375. H3PO4(aq) + OH-(aq) H2PO4-(aq) + H2O(l) H2PO4-(aq) + OH-(aq) HPO42-(aq) + H2O(l) HPO42-(aq) + OH-(aq) PO43-(aq) + H2O(l) Calculate the pH of phosphoric acid solution before any KOH has been added. We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this image
Post Lab Questions 1) If 0.4000 g of KHC&H4O4 are neutralized by 16.58 mL of KOH solution, what is the concentr...

Post Lab Questions 1) If 0.4000 g of KHC&H4O4 are neutralized by 16.58 mL of KOH solution, what is the concentration (molarity) of the KOH solution? KOH(aq)KHCsH4O4(aq) K2CsHa4O4(aq) +H20( 2) What is the concentration (molarity) of 10.0 mL of an H2SO4 solution that is neutralized by 12.97 mL of the KOH solution (use the molarity of KOH you calculated in question 1) H2SO4 (aq)2 KOH(aq)K2SO (aq)2 H20()
A solution of KOH was titrated with 0.1423 g of HBr . If 3.08 mL of...

A solution of KOH was titrated with 0.1423 g of HBr . If 3.08 mL of KOH solution were necessary to neutralize the acid , what was the concentration of the solution ?

4. Solution E was made by mixing 10.0 mL of 0.400 mol/L HBr with 10.0 mL...

4. Solution E was made by mixing 10.0 mL of 0.400 mol/L HBr with 10.0 mL of 0.400 mol/L KBr. The pKa for HBr is –8. A. What is the pH of solution E? B. Solution F was made by adding 1.00 mL of Solution E with 9.00 mL water. What is the pH of Solution F? C. Solution G was made by adding all of Solution F to 10.0 mL of 2.00 x 10-3 mol/L Ca(OH)2. What is the...
In a titration, a student found that 42.6 mL of a KOH solution were required to...

In a titration, a student found that 42.6 mL of a KOH solution were required to neurtralize 28.9 mL of a 0.160 M sulfuric acid solution. Determine the molarity of the KOH solution. SHOW WORK. 2KOH(aq) + H2SO4(aq) ------> K2SO4(aq) + 2H2O(l)
A 20.0-mL sample of 0.400 M HBr solution is titrated with 0.400 M NaOH solution. Calculate...

A 20.0-mL sample of 0.400 M HBr solution is titrated with 0.400 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added. (a) 11.6 mL (b) 15.7 mL (c) 20.0 mL (d) 28.2 mL (e) 33.1 mL

2. A student performs a titration on a 5.00 mL sample of an HBr solution. She...

2. A student performs a titration on a 5.00 mL sample of an HBr solution. She uses 24.32 mL of a 0.459 M KOH solution to reach a phenolphthalein endpoint. (See Example 2, if necessary.) a. Write the balanced equation for the reaction. Remember to include the correct physical states for each reactant and product in your balanced equation. b. How many moles of KOH were used? C. How many moles of HBr were present? d. What is the molarity...