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Part B: Standard pH What color do you see for each sample? Be specific. a. HCl(aq)...
6) A stock solution of HCl is 11.50 M, if 15.29 ml of the stock solution is diluted with water to a total volume of 5.000 L what is the pH, POH, [H3O*], and (OH) at 25°C of the new (dilute) solution? (show your work). pH : рон: [H30*) : [OH') : Experimental Data, Observations, and Calculations - Use correct sig figs and units for all measurements and calculations Part B: Standard pH What color do you see for each...
Part C: Unknown pH 1) What color do you see for each sample? Be specific. a. Unknown 1: Club Soda = b. Unknown 2: Alkaline water = C. Unknown 3: Bleach = d. Unknown 4: Acetate Buffer = e. Unknown 5: Carbonate Buffer= f. Unknown 6: Vodka = 2) Using the ranges of the known substances estimate the pH of each of the unknowns by the color of the red cabbage indicator. a. Unknown 1: Club Soda = b. Unknown...
Tube Order L -> R: 1) Unknown, 2) HCI (aq), 3) H20 (0), 4) NaHCO3(aq), 5) Na2CO, (aq) 6) NaOH (aq) A) Unknown 1: Club Soda B) Unknown 2: Alkaline Health Water C) Unknown 3: Bleach Spray D) Unknown 4: Acetate Buffer HL C) Unknown 3: Bleach Spray D) Unknown 4: Acetate Buffer E) Unknown 5: Carbonate Buffer F) Unknown 6: Vodka Part C: Unknown pH 1) What color do you see for each sample? Be specific. a. Unknown 1:...
12. Given the following: NaOH(aq), pH = 13.301 HCl(aq), pH = 1.000 A mixture is made using 50.0 ml of the HCl and 50.0 ml of the NaOH. What is its pH at 25.0 °C? a. 1.300 b. 7.000 ! c. 12.700 d. 13.000 e. 14.300
(b) Another HCl solution is labeled -0.1 M. What do we know about the pH of this solution? (C) Suppose this sample is tested and the pH meter reads 0.87. Is there a problem with the pH meter or its calibration? Explain. (d) Suppose this same sample is tested and the pH meter reads 2.94. What should you do? 5. A titration of a 20.00 mL sample of 0.1097 M HCl requires 18.86 mL of NaOH to reach the equivalence...
1)A 10.0 mL sample of 0.25 M NH3(aq)
is titrated with 0.20 M HCl(aq) (adding HCl to
NH3). Determine which region on the titration curve the
mixture produced is in, and the pH of the mixture at each volume of
added acid.Kb of NH3 is 1.8 ×
10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the
mixture is [ Select ] ["at", "before", "after"] the
equivalence point on the titration curve.2) The pH of the solution after...
POST LABORATORY QUESTIONS 1. a. For the neutralization reaction that you carried out between HCl(aq) and NaOH (ag). how many moles of NaCl(aq) were produced? b. For the neutralization reaction that you carried out between HCl(aq) and NaOH() how many moles of NaCl(aq) were produced? 2. Calculate AHan for the neutralization of HCl(aq) and NaOH(aq) in kilojoules per mol of NaCl b. Calculate A Hexn for the neutralization of HCl (aq) and NaOH(s) in kilojoules per mol of NaCl 3....
Part I Color changes of Methyl Violet. We will study the following reaction: HMV (aq) + MV (aq) + H* (aq) yellow greenish-blue violet Step 1. Place about 4 mL of distilled water in a regular test tube. Add two drops of methyl violet indicator. Record the color of the solution. Violet Next, add drop by drop, add 6M HCI. This forces equilibrium to be shifted to the left or right-circle the right answer). Adding HCl changes color from to...
What is the pH at equivalence point when HCl(aq) is titrated with NaOH(aq) at 25 °C? 7 1 14 0
QUESTION 14 What is the net ionic equation for: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(1) Option A: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(1) Option B: Option C: Option D: H*(aq) + Cl(aq) + Nat(aq) + OH (aq) → Na*(aq) + Cl (aq) + H2O(1) H*(aq) + OH (aq) → H20(1) Na (aq) + Cl(aq) → Na*(aq) + Cl(aq) O Option A O Option B Optionc O Option D