Abbreviated Report Week 1

Does the number of ions in solution increase, decrease, or remain constant?

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Table 1: Qualitative Analysis of Group II Cations   Group II Cations Confirmatory Reagent Result/ Observation Substance Formed Inference                                                     Write the chemical equations involve in the analysis of group II cations.   Guide Question:   What are differences of the precipitates of each cation in group II?     Reference video : https://www.youtube.com/watch?v=BZGZZx1lHKA

The Solubility Product Constant for zinc phosphate is 9.1 x 10-33 Solid sodium phosphate is slowly added to 125 mL of a 0.0500 M zinc acetate solution. The concentration of phosphate ion required to just initiate precipitation is M. Submit Answer Retry Entire Group 7 more group attempts remaining Submit Answer Use the References to access important values Here The Solubility Product Constant for copper(11) hydroxide is 1.6 x 10-19, Solid sodium hydroxide is slowly added to 50.0 mL of a 0.0340 M copper(II) nitrate solution. The concentration of hydroxide ion M. required to just initiate precipitation is Retry Entire Group 7 more group attempts remaining

please help. will comment and like when all answerd and correct Use the References to access important values if needed for this question. The Solubility Product Constant for calcium fluoride is 3.9 × 10-11. The maximum amount of calcium fluoride that will dissolve in a 0.102 M potassium fluoride solution is Submit Answer Retry Entire Group 8 more group attempts remaining Fil When 25.0 mL of a 1.78 x 10-4 M barium chloride solution is combined with 15.0 mL of a 3.67 x 10-4 M potassium carbonate solution does a precipitate form? ( Kap (BaCO3) = 8.1 × 10-⁹) OYes, the precipitate forms. ONo, the precipitate doesn't form. For these conditions the Reaction Quotient, Q, is equal to When 25.0 mL of a 9.96 x 10-4 M sodium bromide solution is combined with 15.0 mL of a 1.82 x 10-4 M lead nitrate solution does a precipitate form? ( Ksp (PbBr₂) = 6.3 × 10-8) M. OYes, the precipitate forms. ONO, the precipitate doesn't form. For these conditions the Reaction Quotient, Q, is equal to

Procedure 2: • You add cold HCI and notice a white precipitate. • You set the test tube in boiling water and you notice you still have precipitate. You decant the liquid into a different test tube and keep both Procedure 3: • You split the decanted solution in half, into two different test tubes • In the first half, you add potassium chromate into the solution. You notice a yellow precipitate • In the second half, you add sulfuric acid. You notice a white precipitate Procedure 4: • You add ammonia into the test tube. The test tube off-gasses • You then centrifuge the tube. You notice there is no precipitate • To the solution, you add nitric acid until the solution is acidic (which you test with blue litmus paper) • You notice a white precipitate Cations Present, Undetermined, or Absent: Pb: ? Hg: ? Ag: ?

only SELECT correct respomses  1) Titrations of different forms are often employed to quantitate acids, bases, metal ions, and proteins. 2) To perform a titration, the experimenter must be familiar with the stoichiometry of the reaction taking place between the reagent and analyte. 3) Often in titrations, a visible color change will occur in the solution (due to an added indicator solution). 4) Gravimetric titrations directly measure the volume of reagent solution needed to react completely with an analyte. 5) For a monoprotic weak acid titration, the weak acid solution being titrated is the "sample" that is being quantitated. 6) For a monoprotic weak acid titration, the equivalence point is reached when the moles of added base equals the moles of weak acid originally present in the reaction vessel. 7) In a monoprotic weak acid titration, the weak acid is the analyte in solution, and a standardized base (for example, a solution of known concentration of NaOH) is the titrant. 8) A…

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*WRITE RESULTS AND DISCUSSIONS OF TITRATION- CONCENTRATION OF VINEGAR *WRITE CONCLUSION

A solution contains 8.61x10-3 M calcium nitrate and 8.96x10-3 M chromium(III) acetate. Solid ammonium phosphate is added slowly to this mixture. What is the concentration of chromium(III) ion when calcium ion begins to precipitate? [Cr³+] Submit Answer M Retry Entire Group 8 more group attempts remaining A solution contains 1.02x10-2 M zinc nitrate and 1.21x10-2 M silver acetate. Solid potassium cyanide is added slowly to this mixture. What is the concentration of silver ion when zinc ion begins to precipitate? [Ag+] = M

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Quantity Your Data 1.   Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample   5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar   7. Grams of acetic neutralized by the amount of NaOH   8. Percent acetic acid in the vinegar   Hints:     For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value.   For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution.   For #7, Multiply the value obtained in number 6 by the number 1.5.  Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid.   For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…

EM EM 101 App 7-5 ollowing combinations would NOT form a precipitate in aqueous solution? -) Sr(NO:)2 and NaOH )AGNO3 and KBr Zn(C:H3O2)2 and Na:S

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A solution contains 8.38×10-³ M potassium hydroxide and 1.36×10-² M ammonium carbonate. Solid manganese(II) nitrate is added slowly to this mixture. What is the concentration of hydroxide ion when carbonate ion begins to precipitate? [hydroxide] = M Submit Answer Retry Entire Group 2 more group attempts remaining

CHE 1560- General Chemistry II Laboratory Experiment 8: Solubility Product Make Up Assignment BEAKER 2 BEAKER 3 M of NH3 solution 5 M Initial reading of buret 0 mL 10.4 mL (NH3) (mL) Final reading of buret (NH3) 10.4 mL (mL) 19.8 mL Total volume of solution 30.4 mL 29.4 mL after titration Total moles of C2042- Molarity of C2042- Total moles of Cd2+ Moles of [Cd(NH3)42+] Molarity of [Cd(NH3)42+] Moles of NH3 added by titration Moles of NH3 that did not react with Cd2+ Molarity of NH3 that did not react with Cd2+ Kr for [Cd(NH3)42+] Average K for [Cd(NH3)42+]

Correct 5 a and c. Please write them in hand:

Review Homework REQUIRED (NOT Pie Progress) Question 16 of 46 (2 points) | Question Attempt: 1 of Unlimited ✓ 14 15 16 17 18 19 20 21 ✓ 22 ✓ 23 Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A solution B Does a precipitate form when A and B are mixed? empirical formula of precipitate Do ammonium sulfide copper(II) nitrate Oyes no ☐ silver nitrate sodium carbonate O yes no potassium chloride barium nitrate O yes no ☐

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References Use the References to access important values if needed for this question. A solution contains 7.78x10-3 M sodium hydroxide and 1.44x10-² M sodium cyanide. Solid zinc acetate is added slowly to this mixture. What is the concentration of hydroxide ion when cyanide ion begins to precipitate? [hydroxide] = M Submit Answer

Why does it conduct more before and after this minimum point?

3 Solid potassium fluoride is slowly added to 75.0 mL of a 0.233 M calcium bromide solution until the concentration of %. fluoride ion is 0.0632 M. The percent of calcium ion remaining in solution is Submit Answer 20 E $ 4 R F Use the References to access important values if needed for this question. Retry Entire Group % 5 Cengage Learning Cengage Technical Support T G ^ 6 6 more group attempts remaining B Y H ← & 7 U N * 00 8 J ▶ M ( 9 K O ) 0 L P Previous Email Instructor + 11 [ Next> Save and Exit 11 1 d

AaBbCcDd AaBbCcDd AaBbC AaBbCcD AdD AaBb- 1 Normal 1 No Spac... Heading 1 Heading 2 Title Subti 田,、 即咖山 Paragraph Styles 1. 3. 2.15.0 mL HNO3 was titrated to equivalence with 60.0 mL of 0.020 NaOH. What is the concentration of the acid? 近0 of F5 F7 6日 てい いレゴ

A solution contains 7.39x10-³ M sodium carbonate and 6.78x10-3 M sodium phosphate. Solid calcium nitrate is added slowly to this mixture. What is the concentration of phosphate ion when carbonate ion begins to precipitate? [phosphate] = M Submit Answer

HC2H3O2 (aq) + NaOH (aq) ----> NaC2H3O2 (aq) + H2O(l) Trial  Vi (mL) Vf (mL) 1 2.25 15.76 2     3     For their first trial, a student pipettes 5.00 mL of a vinegar solution into an Erlenmeyer flask. The student titrates the vinegar with standardized NaOH with a molarity of 0.317 M. The volume of titrant used was recorded in the table above. Calculate the molarity of the vinegar solution for this trial. Enter a number without units.

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ted Solid manganese (II) sulfate is slowly added to 75.0 mL of a potassium carbonate solution until the concentration of manganese(II) ion is 0.0181 M. The maximum amount of carbonate remaining in solution is M. 80 Submit Answer $ 4 R V % 5 Use the References to access important values if needed for this question. Retry Entire Group 5 more group attempts remaining T G Cengage Learning | Cengage Technical Support ^ 6 B MacBook Pro Y H & 7 N U J ▶ 00 * 8 I M ( - O 9 1 K O Save and Exit ? 1

Pls help ASAP on both questions.