Question

What is the molarity of a solution of HCl if 7.00 mL of the HCl solution...

What is the molarity of a solution of HCl if 7.00 mL of the HCl solution is titrated with 32.4 mL of 0.155 M NaOH solution? HCl(aq)+NaOH(aq)→H2O(l)+NaCl(aq) Express your answer with the appropriate units.

Homework Answers

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
What is the molarity of an HCl solution if 13.0 mL HCl solution is titrated with...
What is the molarity of an HCl solution if 13.0 mL HCl solution is titrated with 26.6 mL of 0.175 M NaOH solution? HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
In a similar conductometric titration, 7.00 mL of an unknown M of NaOH was titrated with...
In a similar conductometric titration, 7.00 mL of an unknown M of NaOH was titrated with 0.115 M HCL. The equivalence point volume was 12.5 mL of HCl. [NaOH (aq) + HCl (aq) --> NaCl (aq) + H2O (l)] (b). Classify the reactants in terms of electrolytes. (c). Classify the products in terms of electrolytes. (d). As the reaction progresses, will the conductivity go up or down? (As products are made and reactants used up, will you have more or...
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...
a) 30.0 ml of an HCl solution of unknown molarity was titrated with .200 M NaOH....
a) 30.0 ml of an HCl solution of unknown molarity was titrated with .200 M NaOH. Phenolphthalien was used as the indicator. The titrated solution turned a very pale pink after 21.8 mL of NaOH was added. What was the initial molarity of the HCl? b)Consider the following three titrations: 100.0 mL of 0.100 M CH3NH2 (Kb = 4.4x10-4) titrated with 0.100 M HCl 100.0 mL of 0.100 M NH3 (Kb = 1.8x10-5) titrated with 0.100 M HCl 100.0 mL...
You determine the concentration of a solution of HCl by titration with NaOH. The titration reaction...
You determine the concentration of a solution of HCl by titration with NaOH. The titration reaction is: HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) Using a volumetric pipet, you transfer 10.00 mL of the HCl solution into an Erlenmeyer flask, then dilute it with ~50 mL of water and add 3 drops of phenolphthalein. The endpoint is reached after you have added 44.00 mL of 0.1250 M NaOH solution from a buret. Calculate the molarity of the original HCl solution....
Part A To what volume should you dilute 20 mL of a 12.0 M H2SO4 solution...
Part A To what volume should you dilute 20 mL of a 12.0 M H2SO4 solution to obtain a 0.130 M H2SO4 solution? Express your answer using two significant figures. Part A Classify the following reactions: HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l) Ba(OH)2(aq)+ZnCl2(aq)→BaCl2(aq)+Zn(OH)2(s) 2AgNO3(aq)+Mg(s)→Mg(NO3)2(aq)+2Ag(s) Drag the appropriate items to their respective bins.
HBr(aq) + NaOH(aq) → H2O(l) + NaBr(aq) 25.00 mL of an HBr solution of unknown molarity...
HBr(aq) + NaOH(aq) → H2O(l) + NaBr(aq) 25.00 mL of an HBr solution of unknown molarity reacts with 28.41 mL of 0.1500 M NaOH. What is the Molarity of the HBr solution?
Determine the volume of 0.150 M NaOH solution required to neutralize each sample of hydrochloric acid....
Determine the volume of 0.150 M NaOH solution required to neutralize each sample of hydrochloric acid. The neutralization reaction is: NaOH(aq) + HCl(aq) → H2O(l) + NaCl(aq) 25 mL of a 0.150 M HCl solution 55 mL of a 0.055 M HCl solution 175 mL of a 0.885 M HCl solution Express your answers, separated by commas, in liters.
HCL reacts with NaCO3 forming NaCl waters and carbon dioxide this equation is balanced as written:...
HCL reacts with NaCO3 forming NaCl waters and carbon dioxide this equation is balanced as written: 2HCl (aq) + Na2 CO3(aq) right arrow 2NaCl (aq) +H2O (l) + CO2)g) 1- what volume of 2.50 M HCL in liters is needed to react completely ( with nothing left over) with 0.750 L of 0.200 M Na2CO3? Express your answer usining Three sig figs and indicate the appropriate units 2- a 531 ml sample of unknown HCL solution reacts completely with Na2CO3...
A volume of 60.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution...
A volume of 60.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 11.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) Express your answer with the appropriate units. Hints Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT