Determine the Concentration of the Unknown Strong Acid In this activity you will use the virtual lab to determine the concentration of a strong monoprotic acid. To do this, you can perform a titration using N2OH and phenolphthalein found in the virtual lab. (Note: The concentration of the acid is between 0.025M and 2.5M so you will need to dilute the N2OH solution so that the volume to reach the endpoint is between 10 and 50 mL). Once you have determined the concentration of the acid, please enter your answer into a form at the bottom of this page. Vịrtual Lab File - Edit - View - Help - OEN Unknown Acid Problem Stockroom Workbench 1 Information Name: PEREZ Unknown Acid Volume: 11.150 mL Temperature: 25.00°C 10.0 M NAOH 25.0 deg 25 mL Pipette 0.0000 mL @ 25.0°C 50.000 mL@ 25.0°C Phenolphthalein 99.850 mL @ 25.0°C 50 mt. Burette 29.000 mt 25.0°C PEREZ Unknown Acid 31.150 mL@ 25.0°C Unknown Acid 90.000 mL @ 25.0°C PEREZ Unknown Acid 11.150 mL @ 25.0°C What is the concentration of the acid (Please use three significant figures for your answer) M.

Determine the Concentration of the Unknown Strong Acid In this activity you will use the virtual lab to determine the concentration of a strong monoprotic acid. To do this, you can perform a titration using N2OH and phenolphthalein found in the virtual lab. (Note: The concentration of the acid is between 0.025M and 2.5M so you will need to dilute the N2OH solution so that the volume to reach the endpoint is between 10 and 50 mL). Once you have determined the concentration of the acid, please enter your answer into a form at the bottom of this page. Vịrtual Lab File - Edit - View - Help - OEN Unknown Acid Problem Stockroom Workbench 1 Information Name: PEREZ Unknown Acid Volume: 11.150 mL Temperature: 25.00°C 10.0 M NAOH 25.0 deg 25 mL Pipette 0.0000 mL @ 25.0°C 50.000 mL@ 25.0°C Phenolphthalein 99.850 mL @ 25.0°C 50 mt. Burette 29.000 mt 25.0°C PEREZ Unknown Acid 31.150 mL@ 25.0°C Unknown Acid 90.000 mL @ 25.0°C PEREZ Unknown Acid 11.150 mL @ 25.0°C What is the concentration of the acid (Please use three significant figures for your answer) M.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Each row or 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. dlo initial type (check all that apply) effect of change on pH (check one) solution initial components change O acidic рH higher H,0, HI add Nal A basic pH lower neutral pH the same acidic pH higher B H,0 basic add K Br pH lower neutral pH the same acidic рH higher H,0 basic add KOH pH lower neutral pH the same acidic рH higher H,0, HI D basic add Na OH pH lower neutral pH the same O OO O OO O O O O
Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________
The Cr3+ concentration in a saturated solution of chromium(III) hydroxide is measured and found to be 1.28×10-8 M. Use this information to calculate a Ksp value for chromium(III) hydroxide.
In this activity you will use the virtual lab to determine the concentration of a strong monoprotic acid. To do this, you can perform a titration using NaOH and phenolphthalein found in the virtual lab. (Note: The concentration of the acid is between 0.025M and 2.5M so you will need to dilute the NaOH solution so that the volume to reach the endpoint is between 10 and 50 mL). Once you have determined the concentration of the acid, please enter your answer into a form at the bottom of this page. Unknown acid: 10 ml 0.15 ml of phenolphthalein 0.60 ml of NaOH
Hydroxyapatite, Ca₁(PO)(OH)₂, Ca₁(PO4)(OH)₂ (s) ⇒ 10 Ca² ¹(aq) + 6PO³(aq) + 2OH(aq) has a solubility constant of Ksp = 2.34 × 10-5⁹, and dissociates according to 10 Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca²+in this solution if [OH-] is fixed at 6.20 x 10-4 M?
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 5 pH = 4 pH = 3 Ca, (PO.), yes O no O yes AgCN O no yes PbCl2 no Explanation Check Accessibili O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy 17 MacBook Air F10 F9 F7 F8 o oo o
Calculate the initial concentration of Fe3+, based on the dilution that results from adding KSCN solution and water to the original 0.0020 M Fe(NO3)3solution. See Step 2 of the procedure for the volume of each substance used in Test Tubes 1-4. This value will be the same value for all four test tubes. This is essentially the same as filling out part of the “I” row in an ICE table. Test tube number 0.0020 M Fe(NO3)3(mL) 0.0020M KSCN(mL) H2O(mL) 1 5 2 3 2 5 3 2 3 5 4 1 4 5 5 0
Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…
6. Open the bags and add 3 drops of bromothymol blue to each bottle. The indicator turns yellow if vinegar is still present and is blue-green when vinegar is not present. Record the color of each solution in the table provided. Data Table 1: Reaction Data Sample 7. Add a 4 teaspoon of baking soda to each bag. Effervescence of CO₂ occurs if excess vinegar is present. Record your observations in the table provided. Moles of vinegar (mol) Moles of baking soda (mol) mistry Relative size of bag Was excess vinegar present? Color with indicator? Reacts with additional baking soda? Moles of gas produced (mol) Watch the limiting reagent! #1 0.042 0.014 чем yes yellow #2 0.042 0.028 #3 yes yellow 0.042 0.042 Experiment 11 yes yellow #4 Stoichiometry 0.042 0.88 more small big bigger bigger No 0.071 #5 NO Geen 0.042 Blue Calculations 1. Use Table 1 to determine which reactant was limiting in each trial. Use the amount of limiting reactant to calculate the moles of carbon dioxide gas that were…
Add 0.3 M AgNO3 to each of the cold sample solutions until AgCl is observed to coagulate. Determine the approximate amount of needed AgNO3 by calculating the volume that would be required if the unknown were pure NaCl.
A phosphate buﬀer solution (25.00 mL sample) used for a growth medium was titrated with 0.1000 M hydrochloric acid. The components of the buﬀer were sodium monohydrogen phosphate and sodium dihydrogen phosphate. The ﬁrst endpoint occurred at a volume of 10.32 mL, and the second occurred after an additional 18.62 mL was added, for a total volume of 28.94 mL. What was the total concentration of phosphate (in any form) in the buﬀer? **Please be as detailed as possible. The different volumes in this titration are a little difficult to understand** THANK you in advance.
A student performed three H2SO4 titrations in Part 2 using their 0.1048 M NaOH solution which they previously standardized in Part 1. They reported the following measurements: Determination #1 Determination #2 Determination #3 Final NaOH Burette Reading 37.65 mL 28.35 mL 26.23 mL Initial NaOH Burette Reading 12.80 mL 4.05 mL 1.73 mL For every 1 mole of H2SO4, how many moles of NaOH are needed to reach equivalence in the titration? Report the integer number only (no units).