7. 33 mL of 3 M HCl is titrated with NaOH to form water and NaCl....

Question

Question

Answer 1

Answer #1

Balanced reaction: HCl(aq) + NaOH(aq) -----> NaCl(aq) + H2O(l)

Number of moles of HCl used in this reaction = 33mL * 3 mole/1000mL = 99*10^-3 mol = 0.099 moles of HCl

As oer the balanced equation, same number of moles of NaOH are needed to neutralize HCl completely.

Thus the answer is option c) 0.099 mol.

Answer 2

Similar Homework Help Questions

Consider the following reaction. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) If 25.0 mL of a...

Consider the following reaction. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) If 25.0 mL of a 0.100 M solution of NaOH reacted with excess HCl, how many moles of NaCl could form? a. 0.00250 mol b. 0.100 mol c. 25.0 mol d. 2.50 mol 1 points QUESTION 9 Consider the following reaction. How many grams of sucrose would produce 2546 kcal? a. 649.4 g b. 1342 g c. 180.4 g d. 1.897 g
20. 25.87 mL of aqueous HCl is titrated to endpoint with 28.16 mL of aqueous NaOH....

20. 25.87 mL of aqueous HCl is titrated to endpoint with 28.16 mL of aqueous NaOH. The NaOH concentration is 0.1146 M. What is the HCl concentration? A) 0.1146 M B) 0.2292 M C) 0.1247 M D) 0.0624 M 21. 13.5 g of NaCl is dissolved in 100.0 g of H20. The boiling point of the water after the salt is added is The boiling point elevation constant for water: K = 0.512 °C/m. A) 102.4° C B) 101.2°C C)...
A 20.00 mL sample of HCl was titrated with the 0.022 M NaOH solution. To reach...

A 20.00 mL sample of HCl was titrated with the 0.022 M NaOH solution. To reach the endpoint required 23.72 ml of the NaOH. Calculate the molarity of the HCI. HCI + NaOH ----> NaCl + H2O Select one: O a. 0.026 M o b. 0.068 M o c. 0.039 M O d. 0.052 M

The reaction of an acid such as HCl with a base, such as NaOH, in water...

The reaction of an acid such as HCl with a base, such as NaOH, in water is an exothermic reaction. HCl(aq) + NaOH(aq) ---> NaCl(aq) + H2O In one experiment, a student placed 55.0 mL of 1.00 M HCl in a coffee-cup calorimeter and carefully measured its temperature to be 35.5oC. To this was added 55.0 mL of 1.00 M NaOH solution whose temperature was also 35.5oC. The mixture was quickly stirred, and the student noticed that the temperature of...
1.) If 15.0 mL of 3.60 M HCl (aq) are added to 10.0 mL of water,...

1.) If 15.0 mL of 3.60 M HCl (aq) are added to 10.0 mL of water, what is the concentration of the resulting solution? 2.) How many mL of water must be added to 25.0 mL of a 0.500 M NaCl solution to result in a solution that is 0.200 M NaCl? 3.) The net ionic equation for the reaction of aqueous solutions of sodium chloride and silver nitrate is...? 4.) How many mL of a 0.500 M sodium chloride...
1. If 40.00 mL of 0.050 M HCl is titrated with 0.100 M NaOH, what is...

1. If 40.00 mL of 0.050 M HCl is titrated with 0.100 M NaOH, what is the pH at the following "times?" (9 pts) a. Before any NaOH is added. b. After 20.00 mL of NaOH is added. c. After 500 mL of NaOH is added. 2. If 50.00 mL of 0.050 M formic acid, HCHO, (yes, you need to look up the Ka for formic acid) is titrated with 0.050 M NaOH, what is the pH at the following...

HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(1) 100.0 mL of 0.500 M HCl is mixed with...

HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(1) 100.0 mL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M NaOH in a coffee cup calorimeter. Assuming the temperature of the solution was initially 25.0 °C, and the final temperature of the solution was 26.7 °C, calculate the enthalpy of this reaction per mole of HCl. Assume the density of the water and acid and base solutions are all 1.00 g/mL.
Write the balanced equation occurring between HCl(aq) and NaOH(aq). a. It takes 15 mL of 0.125...

Write the balanced equation occurring between HCl(aq) and NaOH(aq). a. It takes 15 mL of 0.125 M NaOH to reach the end point of the reaction. How many moles of NaOH have you added? b. What is the mole ratio between HCl and NaOH? How many moles of HCI were in the titrated sample? c. At the beginning of the titration, there were 22 mL of HCl. What was the original concentration of HCl?
If 32.12 mL of 3.77 M hydrochloric acid solution, HCl, are titrated with 51.5 mL of sodium hydroxide solution, NaOH...

If 32.12 mL of 3.77 M hydrochloric acid solution, HCl, are titrated with 51.5 mL of sodium hydroxide solution, NaOH, according to HCl(aq) + NaOH(aq) - NaCl(aq) + H2O(1) what is the concentration of the sodium hydroxide solution? (Enter your

A titration of 25.00 mL of O.1550 M HCl solution with a solution of NaOH of...

A titration of 25.00 mL of O.1550 M HCl solution with a solution of NaOH of unknown molarity starts at a buret reading for NaOH of 0.33 mL The phenolphthalein indicator turns light pink the acid solution for over 30 seconds at a buret reading of 24.19 mL 2) What was the volume of HCl you started with? 3) How many moles of HCl were in the original solution? 4) Write the balanced chemical equation for the titration reaction. 5)...