BIO202L Lab Exam 15

I need help calculating the initial concentrations please.

15 - #10. Thumbs up if you do it correctly! MAKE SURE TO HAVE THE CORRECT SIGNIFICANT FIGURES IN YOUR FINAL ANSWER.

Graph data with Concentration on the x-axis and Absorbance on the y-axis. Find the line of best fit for your data points. Record the respective formula in y=mx+b.

Please submit answers with correct number of Significant figures

An aqueous solution is found to have an OH- concentration ( [OH-] ) of 1.0 x 10-8 M. You can assume that kW = 1.0 x 10-14.   Select all the correct statements about this solution.   An aqueous solution is found to have an OH- concentration ( [OH-] ) of 1.0 x 10-8 M. You can assume that kW = 1.0 x 10-14.   Select all the correct statements about this solution.   The solution is basic. The solution is acidic. The pH of the solution is 8.00 The pH of the solution is 6.00 The pOH of the solution is 8.00 The pOH of the solution is 6.00 The concentration of the hydronium ion, [H3O+], is 1.0 x 10-6 M. The concentration of the hydronium ion, [H3O+], is 1.0 x 10-8 M.

Pls help ASAP ON ALL ASKED QUESTIONS PLS PLS

- 14 + An aqueous solution at 25 °C has a OH concentration of 3.4 × 10 M. Calculate the H₂O* concentration. Be sure your answer has 2 significant digits. M Dx1 x10 Ś

Can someone please help?

Sample 1 A student states “A solution of 4 M sulfuric acid (H2SO4) is a stronger acid than a 1 M solution of sulfuric acid.” Construct a well-thought out response to help this student improve his understanding.   Sample 2 Draw and upload representation that shows 10 molecules of a weak acid dissolved in water with 20% ionization. Include only the water molecules that react, not the excess water molecules in the solution.   Sample 3 You have conductivity meters in 1 M solutions of HNO3, HNO2, and HC2H3O2. The 1 M HNO3 light bulb is bright, the 1 M HNO2 light bulb is giving off some light, and the 1 M HC2H3O2 is very dim. Rank the solutions in order of acid strength based on this information. (Strongest, middle, weakest)

to 2 significant digits, and Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for your entries for pH to 2 decimal places. solution [10] -7 PH [H₂O] to A 4.2 x 10 B mol/L mol/L ☐ 5 1.22 -10 2.8 x 10 mol/L C ☐

› Phthalic acid (H₂CH₂O4) is a diprotic acid with Kal = 1.12 x 10-³ and K ₁2 = 3.90 x 10-6. Determine the pH of each solution. A 0.294 M phthalic acid (H₂CH₂O) solution. pH = = A 0.294 M sodium phthalate (Na₂ CH₂O₂) solution. pH =

Part 1 of 2 Determine the pH of a 0.25 M NH3 solution. Be sure your answer has the correct number of significant digits. Note: K for NH3 is 1.78 × 10-5 pH = Part 2 of 2 x10 Determine the pH of a solution that is 0.25 M NH3 and 0.35 M NH4Cl. Be sure your answer has the correct number of significant digits. pH = X

Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for H,O to 2 significant digits, and your entries for pH to 2 decimal places. [1,0] solution pH x10 12 A 7.1 x 10 mol/L mol/L 0.090 8.4 x 10 mol/L

ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?

. Fill the flask to the Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. Calculating the pH of a weak acid solution The acid dissociation constant K of boric acid (H₂BO3) is 5.8 × 10-¹0. Calculate the pH of a 4.4M solution of boric acid. Round your answer to 1 decimal place... Calculating the pH of a weak base solution The base protonation constant K of ammonia (NH3) is 1.8 × 10-5. ०.१५ Calculate the pH of a 0.94 M solution of ammonia at 25 °C. Round your answer to 1 decimal place. TEXAS INSTRUMENTS TI-30X 100000000

using table 1, answer the questiosn below.  Mass of Crushed Antacid (g) .500g Concentration of HCl (M) 1.0 M Volume HCl (mL) 5.01ml Concentration of NaOH (M) 1.0M Initial NaOH Volume (mL) 4.10ml Final NaOH Volume (mL) 2.60ml Total Volume of NaOH Used (mL) 1.5ml   HCl available for neutralization (g): Moles of NaOH required to reach stoichiometric point (mol): HCl neutralized by antacid (g): HCl neutralized per gram of antacid (g):

In a 0.73 mM aqueous solution of 4-chlorobutanoic acid (C,H¸CICO,H), what is the percentage of 4-chlorobutanoic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. 0% x10

9. A solution of 40ml containing 15 grams of sodium hydroxide is analyzed. a. What is the concentration of the solution? O 4.7M 10 M 3.7 M 9.4 M 8 00:56:26 PREVIOUS 9 of 9 SAVE & esc 2

- 10 M. Calculate the OH concentration. Be sure your + An aqueous solution at 25 °C has a H,O' concentration of 2. × 10 answer has the correct number of significant digits. | M x10

Acid Data table Initial volume of Vinegar Percent acetic acid in vinegar sample HG mc Base Data table mol base = mol acid I mol acid Imol base Concentration of NaOH solution 0125 M Initial volume of NaOH in buret 12.50 ml 0.98 Post-Activity questions 15.30 ML Mol of acetic acid 10.016 mol Final volume of NaOH in buret 54.00mL 50.ML 41.90mL n mol acid 0.016E am Slov mol acce Molacid 16m² yoland (2) 0.016 Molarity of Acetic acid 10.994 M. Mol NaOH added. 51.5 49.12 12616 1. Does your molarity of acetic acid agree with the percent of acetic acid present in the sample? Use a calculation to determine this 2. At what pH does phenolphthalein turn pink? Do you think this causes an error in the measurement of the equivalence point? 3. Describe how determining the titration of an unknown base with a known acid using phenolphthalein as an indicator would differ from our titration today. Discussing the expected changes in color would from phenolphthalein would be a good way to frame your answer.

9. What is the concentration of hydronlum (H0), the pH is 1.257 Write your answer to 3 significant figures in decimal form. Type your answer. 10 What is the concentration of hydroxide OHir the concentration of hydronium is HsO 4.698 x 10 MISolve to 3 signiicant figures and use decimal form. Type your answer.

What is the molarity of an aqueous solution that contains 0.0720 g C2H6O2 per gram of solution . The density of the solution is 1.04 g/mL X STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 1.04 62.08 6.022 x 1023 0.0720 1.21 x 10-3 4650 1.12 1000 1.21 1 0.001 g C2H.O2 mol C2H6O2 g C2H&Oz/mol g solution/mL mL solution g C2H6O2/g solution M C2H6O2 L solution g solution

The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms.pH = - log [H+] where [H+] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.99 x 10-3 mol/L, the pH is ______.b. If the pH of a solution is 3.441, the hydrogen ion concentration is ________ mol/L.

The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = − log [H+] where [+] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 4.92 × 10-³ mol/L, the pH is b. If the pH of a solution is 3.078, the hydrogen ion concentration is mol/L.

Fill in the table rows. Maintain the same number of significant digits. pH [H+] [OH]] РОН 1.9 4.73 1.0 x 10-7 M 2.1 M

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For water and wastewater engineering. This is for a review I made, not for a grade. Please show equations and choose and answer choice.

Help me answer all the empty boxes in the following table:

How many milliliters of 0.105 M HCl are needed to completely neutralize 40.0 mL of 0.108 M Ba(OH)2 solution? Express the volume in milliliters to three significant digits. V = %3D mL Submit Request Answer