Lab 14 Handin done

1. Calculate the theoretical molarity of 100ml of a 0.10 M NaOH solution. 2. Calculate the actual molarity of the NaOH solution that you prepared. 3. Calculate the percent error between the two NaOH values above.

EXPERIMENT 10 PRE-LABORATORY QUESTIONS STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0.50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155

1. Calculate the theoretical molarity of the NaOH solution you prepared. 2. Calculate the actual molarity of your .10 M NaOH solution. 3. Calculate the percent error between the two NaOH values you have.

I need help please calculating the values!

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change effect of change on pH (check one) acidic A H₂O basic add NaNO3 neutral acidic O pH higher pH lower pH the same O pH higher B H₂O, HCI basic add K Cl O pH lower neutral acidic C H₂O, HCI basic add KOH neutral acidic D H₂O basic add HNO3 Oneutral O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same 5

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Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type (check all that apply) solution initial components effect of change on pH (check one) change O acidic O pH higher H,0, H Br O basic add KOH O pH lower neutral pH the same O acidic pH higher H,0 O basic add Na OH pH lower neutral pH the same O acidic pH higher H,0 O basic add NaI O pH lower O neutral pH the same acidic pH higher H,0, H Br O basic add K Br pH lower pH the same O neutral Exnlanation Check 2021 McGraw-Hill Educa

I need help with question 3?

Help me answer this one question:

For propanoic acid (HC3H502, Ka = 1.3 x 10-5) Determine the percent dissociation of a 3.42 M solution. % Question Help: Message instructor Submit Question AUG 19 80 F3 000 000 F4 % 95 54 #3 ķ 649 119 F5 F6 F7 6 27 & 8

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Question 16 I want a detailed explanation thanks

Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins? (Two decimal places) Type your answer...

10.0 mL 0.5 M HCl neutralizes ________ mL 0.1 M NaOH.

Question 18 of 30 Submit A 20.0 mL solution of NaOH is neutralized with 26.3 mL of 0.200 M HBr. What is the concentration of the original NaOH solution? | M 1 4 6. C 7 +/- x 10 0 Tap here or pull up for additional resources 3. LO 00

Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH when 10.00 mL of HBr have been added? (Two decimal places) Type your answer...

How many mL of 0.15 M NaOH would be required to titrate 35.0 mL of 0.12 M H2$O4? 2 NaOH + H2$O4   (arrow ) Na›SOs +2 HO

Calculate the %(m/v) of hydrochloric acid using the molar concentration you found. Shows calculations. Records final answer to correct significant digits. Records the concentration with the appropriate units. The molar concentration I found was 0.1M.

A student performs a titration on a 5.00 mL sample of an HBr solution. She uses 24.32 of a 0.459 M KOH solution to reach a phenolphthalein endpoint. Answer the following questions below.

Please help me answer this question:

How to calculate the molarity of the acetic acid. And how to calculate the grams of acetic acid in 1 liter of the vinegar.

Please answer the 3 boxes for ph

PRE-LAB QUESTIONS Calculate the volume, in mL, of a 0.50 M NaOH solution that will be required to titrate 1.2 g of potassium hydrogen phthalate to the phenolphthalein end point. The molar mass of KHP is 204.2 g/mol. 1.

A-2 Sodium Carbonate + HCl Please answer the question and part a. 1) Observations on adding 5 drops of 6 M HCl to 2 Ml of saturated Na2CO2 solution: a) Balaced chemical Equation:

o explain how the result of a titration is affected if you titrate past the end point, calculate the percentage error for one drop past the end point of a 30 mL titration, using a 0.100M NaOH titrant. (Note: The volume of 20 drops is equal to 1 mL.) Select one:a. % error=0.1%;b. % error=0.3%;c. % error=0.2%;d. All options are incorrect;e. % error=0.4%;