1.If 23 ml of 2.0 M NaOH was required to neutralize 10.0 ml of HCl, what is the molarity of the HCl?
2.What volume (in L) of a 2.08 M NaOH solution is required to neutralize 0.53 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?
1.If 23 ml of 2.0 M NaOH was required to neutralize 10.0 ml of HCl, what...
Question 40 of 65 > The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.140 M NaOH. It requires 12.8 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? concentration: MHCI
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)...
stion 62 of 65 > The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.320 M NaOH. It requires 19.4 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? CH concentration: 1.6 M HCI Incorrect 63 of 65 > A barium hydroxide solution is prepared by dissolving 1.67 g of Ba(OH), in water to make 33.6 mL of solution. What is...
The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.210 M NaOH. It requires 16.4 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? concentration: MHCI URILE
3. A student pipetted 25.00 mL of a 0.2531 M solution of HCl into an Erlenmeyer flask. After adding 3 drops of phenolphthalein indicator to the flask, the student started adding NaOH from the burette, until the color in the Erlenmeyer flask turned light pink, The student calculated that 21.40 mL NaOH was transferred in the flask to neutralize the acid. a) Calculate the number of moles of HCl initially present (Reaction: NaOH(aq) + HCl(aq) -NaCl(aq) + H2O() b) Calculate...
11.83 mL of 0.5008 M NaOH was required to neutralize 25.00 mL of HCl with unknown molarity. How many moles per liter of NaOH was used?
9.) What volume of 0.750 M HCl is required to neutralize 10.0 mL of 1 M NaOH? Show your work. 10.) How many grams of CoHi20s are present in a 250 mL. solution with a concentration of 0.123 M? Show your work
what is the molarity of HCl solution molarity of NaOH: .5046 Begin by prepa. Titration of the Trial 5 Trial 6 ve 2: Titration of the Unknown Acid Weigh ou Trial 4 flask - Volume of acid acquired: 10.0 10.0 10.0 Initial buret reading: 1.48 8.58 15.87 8.58 15.87 22.97 Final buret reading: *Volume of NaOH solution used: 7.10mL 6.99 mL 7.10mL *Molarity of HCI solution: Show your calculations here:
Amy prepared her base solution by adding 16 mL of 6.1 M NaOH to her 500 mL bottle and then filling it to the shoulder. She then standardized her base solution by titrating it with a 0.216 M HCl solution. She filled one buret with her NaOH solution and another buret with the HCl solution. The initial readings on the burets were 1.74 mL (NaOH) and 1.43 mL (HCl). She then dispensed some HCl into an Erlenmeyer flask, added a...
A buret is filled with 0.1517 M NaOH(aq). A 25.0 mL. portion of an unknown acid HA(aq) and two drops of indicator are added to an Erlenmeyer flask, and the titration experiment is carried out. The initial buret reading was 0.55 ml., and the buret reading at the end point was 22.50 mL. How many moles of NaOH(aq) were dispensed during the titration? O 21.95 mol O 3.33 mol O 3.33 x 10 mol O 3.330 x 10 mol O...