Abbreviated Report Week 1

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

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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

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…

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

please answer in text form and in proper format answer with must explanation , calculation for each part and steps clearly

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

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

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

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Please don't provide handwritten solution

52 Types of Chemical Reactions 3) Get a clean dry medium test tube and add a small amount of calcium oxide solid to it. Now add enough deionized water to cover the solid in the test tube and test the resulting mixture with universal indicator. What does the color of the universal indicator tell? Balanced chemical equation: 4) Get a medium test tube and fill it with about 5 mL of water and a few drops of universal indicator. Take a soda straw and gently blow bubbles into the water. Note what happens to the color of the universal indicator. What does the color of the universal indicator tell? Balanced chemical equation:

14. Iodine Yellow: Pb(NO3)2 (aq) + Nal (aq) Names: lead (1) nitrate Colors: Colorless Species Initially Present: Evidence of Reaction: and sodium toriely lodide and colorless mustard yellow. 3- Pb No, Nat, I Name and Balanced Net Ionic Equation for Precipitation: 15. New Pigment Formulation... Combine equal volumes of two reagents to prepare a precipitate n included in the previous reaction mixtures. Cobalt (11) Names: Chloride and barium chlorid Colors: pink and miky white Species Initially Present: Bart, CT, 8 Co+, CT Evidence of Reaction: Name and Balanced Net Ionic Equation for Precipitation: rose Pink

Number 1

Please correct answer and don't use hend raiting

[Review Topics] [References] Use the References to access important values if needed for this question. A solution contains 1.24x10-² M silver nitrate and 9.41x10-³ M calcium acetate. Solid ammonium sulfite is added slowly to this mixture. What is the concentration of silver ion when calcium ion begins to precipitate? [Ag+] = M Submit Answer Retry Entire Group 2 more group attempts remaining

Please help with on the guide questions section below.  Thank you.

Part A A solution contains 2.3x10-4 M Ag+ and 1.7x10-3 M Pb2+ Part B Specify the concentration of I needed to begin precipitation. Express your answer using two significant figures. ΜΕ ΑΣΦ 0 ? 4.2.10 - 13 Submit Previous Answers Request Answer M

Make sure has correct significant di

balanced molecular equation (ME)  write the balanced complete ionic equation (CIE)  and write the balanced net ionic equation (NIE) Copper(II) nitrate  +  potassium hydroxide           Cu(NO3)2(aq)                 KOH(aq)       Observations:  Blue gelatinous precipitate       ME:         CIE:        NIE:

Titrant: It is the solution that is placed in the burette :Select one True False

II only O both I & II ОШ only QUESTION 13 Consider an acid-base titration in which the base is dispensed from a burette into a flask containing an acid. If any drops of the base adhere to the inner walls of the flask, but do not actually mix with the solution, the calculated acid concentration would be O the same as the actual value. O lower than the actual value. O higher than the actual value. Need more information Click Save and Submit to save and submit, Click Save All Answers to save all answers. Save Al

A student performed titration to find the concentration of acetic acid. Titrant was sodium hydroxide. He went beyond the indicator color change by adding too much titrant. How will his experimental error affect the calculated value for the concentration of unknown acetic acid? calculated value actual value. calculated value < actual value calculated value = actual value. more information is necessary this is not a source of error

Please use the values in the resources listed below instead of the textbook values. Calculate the concentration (in M) of Agt when AGIO, just begins to precipitate from a solution that is 0.0325 M in IO,. (Ksp = 3.17×10-8) %D 4.0 Supporting Materials Periodic Table Constants and Supplemental Data Factors Additional Materials Section 15.1 MacBook Air 吕0 888 F1 F2 F3 F4 F5 F6 F7 F8 F9 @ 2$ & 1 2 3 4 5 7 Q W E R Y 00 T

A solution contains 8.38×10-³ Μ potassium hydroxide and 1.36×10-² Μ 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