▾ Part A Write a chemical equation that illustrates the autoionization of water. Express your answer as a chemical equation. Identify all of the phases in your answer. Templates Symbols undo' rego reset keyboard shortcuts Help A chemical reaction does not occur for this question. Submit Previous Answers Request Answer
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- Table 12.9 (data) Buffer Initial pH pH after adding HCI pH after adding NaOH 6 8 6 4 Solution A 5-6 8 Solution B8-9 10 Solution C7 9-10 Solution D 5 Boiled distilled water 5 9-10 4 9 Table 12.10 (report) Solutions able to buffer well against acid Solutions able to buffer well against base Solutions able to buffer well against acid or base Solutions with little or no buffering ability against acid or base# ? The volume of water needed to dissolve 0.0674 grams of calcium sulfate is Assume no volume change upon addition of the solid. 80 Submit Answer 54 $ 4 000 000 [Review Topics) [References] Use the References to access important values if needed for this question. Retry Entire Group % 5 more group attempts remaining Cengage Learning Cengage Technical Support MacBook Pro 6 4 & 7 ▶II * 00 61 9 ) O- 1 L. Email Ins I (Pre JPart B - Carbonate Equilibrium Part B - Carbonate Equilibrium 1. Choose a wide test tube from your locker to use as tube A in the apparatus shown on the right. Add 2 M HNO3 to the test tube to a depth of about 2 CO,(g) cm, then add tap water to half-fill the tube. Let it soak with a little stirring for 30 seconds, then empty the acid into the sink. Rinse the test tube with Tube B PROCEDURE OBSERVATIONS EQUATIONS side-arm Pliable vinyl tubing test tube LOTS OF WATER (rinse under running water in the sink). Initial bubbling of CO2(g) (Step 4) (immediate change) Tube A 2. Pour about 20 mL of saturated Ca(OH), solution into this test-tube (tube A in diagram on right). If the saturated Ca(OH), solution is cloudy you may need to filter it into the tube. Ask your demonstrator if filtration is required. Saturated calcium hydroxide CO(S) solution 3. Place several small pieces of dry ice into test-tube B. Fit the cork into test Addition of excess CO2(g) (Step 5) (second observable change) tube B…
- Tab Window Help age Learning X ATM HOMEWORK Module 9 X Submit Answer Mind Tap - Cengage Learning X loymentid=5735112480241329813180832311&eISBN=9781305862883&id=1707786068&snapshotid=33225... References Use the References to access important values if needed for this question. dation-Reduction Titrations: This is group attempt 1 of 10 tv Suppose a solution of the reducing agent Cut is titrated with a solution of the oxidizing agent permanganate. The balanced net ionic equation for the reaction is: MnO4 (aq) + 5Cu*(aq) +8H30*(aq) →Mn²+ (aq) + 5Cu²+ (aq)+12H₂O(l) What volume (in mL) of a 0.1258 M MnO4 solution would be required to consume the Cu* in a 20.00 mL sample of a solution containing 0.5548 M Cu*? mL Numeric input field Autosaved at 10:58 PM a 8 C G What volume (in mL) of a 0.125 A WWrite the Ksp expression for the sparingly soluble compound silver cyanide, AgCN. If either the numerator or denominator is 1, please enter 1. Ksp = Submit Answer Retry Entire Group 8 more group attempts remaining6. 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…
- For the CO2 impact experiment station: 1) Obtain two plastic cups, red cabbage indicator, a straw, and plastic wrap. 2) Fill each cup approximately one-quarter to one-third full of tap water and add ~10 mL of the red cabbage indicator. 3) Place the two cups side by side on a sheet of white paper. 4) Place the straw into one of the beakers and cover that beaker with the plastic wrap. 5) Carefully blow bubbles into the test cup for 3 min. and observe both cups. 6) Compare the color to the control cup and record any differences. This the Question: Did the beaker with the solution into which CO2 was bubbled change pH/color? By how much? Is this what, you would predict, based on your knowledge of the chemistry of CO2?O KINETICS AND EQUILIBRIUM Calculating the solubility of an ionic... Calculate the solubility at 25 °c of CaF₂ in pure water and in a 0.0200M NaF solution. You'll find ê data in the ALEKS Data tab. sp Round both of your answers to 2 significant digits. solubility in pure water: ㅁ은 solubility in 0.0200 M NaF solution: 0 60- 0 x10 X 0x0 1/3 00all i need is help with question 4 a !!
- Fill in the "Reactions" in the provided Data Table I've already tried to complete most of the table. Need you to check the reactions I have + I'm not sure what the reaction is for the second box (I left it blank) The procedure is attached and a flow chart Sample Procedure Observation for Known (Week 1) Chemical Equation(s) Observation for Unknown (Week 2) Conclusion for Unknown (Week 2) Part A Step 1 & 2 & 3 Solution (acidified with HNO3) + 12M HCL (2 drops) + 6M HCL (2 drops) White precipitate: precipitate washed (step 6) supernatant saved for Part B Reactions: 1. Ag+ + Cl- → AgCl(s) 2. Hg22+ + 2Cl- → Hg2Cl2(s) 3. Pb2+ + 2Cl- → PbCl2(s) White precipitate Pb2+, Hg22+, and Ag+ possible Part A Step 7 & 8 Precipitate + hot H2O (10 drops) Some precipitate dissolves into solution supernatant for step 9 precipitate for step 10 Reaction: 1. Remaining precipitate = Part A Step 9 Supernatant + 2 drops of 1M K2CrO4…The course is specifically quantitative analysis, I figured that would just fall under chemistry. The issue I'm having with this one is that I have absolutely no idea how to even begin. I figure benzoic acid wouldn't affect the pH of NaOH that much since it's a weak acid and NaOH is a strong base, but I don't think it'd be right to just take the pH using solely the concentration of NaOH. What approach should I take to solve this? 220 mL of 0.03 M NaOH were added to 200 mL of 0.03 M benzoic acid (pKa = 4.2). What is the pH of the resulting solution?how do you do this question? this is a non graded practice worksheet