Question

1) What kind of acid is the active component in "The Works" toilet bowl cleaner? 2)...

1) What kind of acid is the active component in "The Works" toilet bowl cleaner?

2) If 23 ml of 1.4 M NaOH was required to neutralize 10.0 ml of HCl, what is the molarity of the HCl?

3) What volume (in L) of a 2.12 M NaOH solution is required to neutralize 0.16 mol of HCl?

*Remember to report your answer using the proper significant digits

4) A student has finished the titration of a sample of HBr of unknown concentration with 0.2 M NaOH. The student notices small drops of unreacted NaOH were left on the neck of the flask. This means that these drops were dispensed from the buret but were not mixed with the HBr. How will this affect the calculated molarity of the HBr acid?

a)

Cannot be determined

b)

The calculated molarity will be higher than the actual molarity of the unknown.

c)

The calculated molarity will be lower than the actual molarity of the unknown.

d)

This will have no effect on the calculated molarity.

Homework Answers

Answer #1

Q1

this is mainly hydrochloric acid at a 9-11% mass concentration

Q2

mmol of base = MV = 1.4*23 = 32.2

ratio is 1:1 so

mmol of acid = 32.2

[HCl] = mmol acid/V = 32.2/10 = 3.22 M

Q3

find V of NaOh for a 0.16 mol of HCl

mol of HCL = 0.16

molof NaOH required = 0.16 mol

then

M = mol/V

V = mol/M

V = 0.16 * 2.12 = 0.3392 L

V = 339.2 mL

Q4

the volume of base will be higher, therefore molarity of HBr will be highier ( incorrectly)

so the concentration will appear to be higher

choose B

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1) What kind of acid is the active component in "The Works" toilet bowl cleaner?​ 2)If...
1) What kind of acid is the active component in "The Works" toilet bowl cleaner?​ 2)If 33 ml of 1.7 M NaOH was required to neutralize 10.0 ml of HCl, what is the molarity of the HCl? 3) What volume (in L) of a 1.16 M NaOH solution is required to neutralize 0.56 mol of HCl? *Remember to report your answer using the proper significant digits 4) A student has finished the titration of a sample of HBr of unknown...
1. When a 0.5725 g sample of Lysol toilet bowl cleaner was titrated with 0.100 M...
1. When a 0.5725 g sample of Lysol toilet bowl cleaner was titrated with 0.100 M NaOH, an end point was obtained at 15.00 mL. Calculate the percent (by weight) of hydrochloric acid in the Lysol sample. b. When a 3.529 g sample of Liquid-Plumr was titrated with 0.100 M HCl, two end points were obtained. The first end point occured at 15.0 mL, the second at 42.00 mL. Calculate the percentages of both NaOH and NaOCl in Liquid-Plumr.
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) 4.00 mL of an unknown...
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) 4.00 mL of an unknown acid solution containing HCl was added to flask containing 30.00 mL of deionized water and two drops of an indicator. The solution was mixed and then titrated with NaOH until the end point was reached. Use the following titration data to determine the mass percent of HCl in the acid solution. Mass of flask: 125.59 g Mass of flask + acid solution: 129.50 g...
The following questions involve the reaction of sodium hydroxide and succinic acid. Succinic acid is diprotic:...
The following questions involve the reaction of sodium hydroxide and succinic acid. Succinic acid is diprotic: the acid (H2C4H4O4) reacts with two of its hydrogens to give C4H4O42-. The balanced "molecular" equation for the reaction has coefficients of 2 for NaOH and 1 for succinic acid: 2 NaOH (aq) + H2C4O4 (aq) --> Na2C4H4O4 (aq) + 2 H2O (l) A student weights 1.700 g of succinic acid and dissolves it in water in a 250.0 mL volumetric flask. A 25.00...
A chemist is determining the molarity of unknown acid by adding enough base with a buret...
A chemist is determining the molarity of unknown acid by adding enough base with a buret to reach the equivalence point. The initial buret reading that contained the NaOH was 3.45 mL (+/- 0.02 mL) and the final reading was 28.91 mL (+/- 0.02 mL)   The molarity of the base was labeled as 0.078 M (+/- 0.0004). How many moles of base were added to the flask, report to the correct answer as indicated by absolute uncertainty.
Molarity of NaOH: 0.1388 M Unknown Acid Buret: Trial 1 Trial 2 Initial Buret Reading 27.11...
Molarity of NaOH: 0.1388 M Unknown Acid Buret: Trial 1 Trial 2 Initial Buret Reading 27.11 ml 17.91 ml Final Buret Reading 47.31 ml 42.01 ml Volume of acid added 20.10 ml 24.10 ml Results: Trial 1 Trial 2 Volume of NaOH at equivalence point 4.75 mL 14.03 mL Volume of NaOH at one-half the equivalence point 2.37 mL 7.015 mL pH at half equivalence point 4.88 4.21 pKa of unknown acid Average pKa Average Ka Moles of unknown acid...
6. Consider the following balanced acid/base reaction: 2 CH3COOH +   Ba(OH)2 -> (CH3COO)2Ba   + 2 H2O...
6. Consider the following balanced acid/base reaction: 2 CH3COOH +   Ba(OH)2 -> (CH3COO)2Ba   + 2 H2O A student pipetted 5.00 mL of a 0.224M solution of CH3COOH into an Erlenmeyer flask. The student calculated that 36.44 mL Ba(OH)2 was needed to neutralize the acid. Calculate the molarity of Ba(OH)2 in the unknown solution.               7. In an aqueous solution the [H3O+] is 2.77x 10-9.M.            a. Is this solution acidic, basic or neutral?         b. What is the...
1.)Rank the given compounds based on their relative Brønsted acidities. H-F, H-CH3, H-SH, H-NH2, H-CL 2.)...
1.)Rank the given compounds based on their relative Brønsted acidities. H-F, H-CH3, H-SH, H-NH2, H-CL 2.) Write the chemical equation for the reaction of carbonic acid (H2CO3) with water. 3.) The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.250 M NaOH. What volume of NaOH is needed to reach the end point of the titration? What was the initial concentration of HCl?
1.Write the molecular equation and the net ionic equation for the reaction of H2SO4 with NaOH....
1.Write the molecular equation and the net ionic equation for the reaction of H2SO4 with NaOH. 2. Exactly 25.00 mL of 0.1522 M H2SO4 were needed to titrate 45.25 mL of NaOH according to the balanced equation in the problem above. Calculate the moles of NaOH needed for the reaction. Calculate the molarity of the NaOH solution. 3. One group of students made an error by using HCl instead of H2SO4 to titrate an unknown solution of NaOH. Would this...
Procedure Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare...
Procedure Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare the NaOH Solution Take a 250 mL volumetric flask from the Containers shelf and a balance from the Instruments shelf and place them on the workbench. Zero the mass of the volumetric flask on the balance. Take sodium hydroxide from the Materials shelf and add 1 g to the flask. Record the mass from the balance display. Place the volumetric flask on the workbench....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT