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

What volume of 0.250 M NaOH is required to react completely with 0.0100 moles of H2SO4? (a) 80.0 mL (b) 60.0 mL (c) 40.0 mL (d) 125 mL

You need to make 150.0 mL of a 0.10 M NaCI solution. You have solid NaCl, and your lab partner has a 2.5 M NaC1 solution. Explain how you each independently make the solution you need.

7:21 1 4 7 +/- Question 8 of 13 A 20.0 mL solution of NaOH is neutralized with 22.8 mL of 0.200 M HBr. What is the concentration of the original NaOH solution? 2 5 8 M 3 60 9 O Submit Tap here or pull up for additional resources XU x 100

(10 ||| 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. Microsoft O Predicting precipitation W Microsoft Microsoft 6.52.210... esc solution A zinc nitrate iron(II) iodide iron(II) nitrate Explanation 5 T C solution B ammonium sulfide zinc nitrate potassium hydroxide Check 9,216 280 #m Does a precipitate form when A and B are mixed? 103 yes NOV 1 yes O yes no $ 4 no no OOO % Q Search or enter website name LO empirical formula of precipitate 5 0 0 stv 6 X & 7 5 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility * 00 8 A ( 9 W 0 DOCX – + 11 { olo Ar 2 lal h Eng

As part of this experiment you will need to determine the concentrations of Fe* and SCN ions present in test tubes 1-9. These values can be calculated using the volumes and concentrations provided in Tables 1 and 2 of the Equilibrium Lab - Procedure and the dilution equation (M,V1 = M2V2). Note: the solutions provided in the lab, and therefore the tables in the lab document, are the compounds used to prepare the solution. You must determine the concentration of the ions based on how these compounds díssociate in solution Complete the following table by filling the the calculated initial concentrations of each substance. Be sure to: Pay attention to significant figures • Round appropriately Use decimal notation (not scientific) Do not include units Test Initial [Fe3*] (M) Initial [SCN'] (M) Tube 1 3 4. 6. 7 8. 2.

A standard solution of a chemical compound was prepared by diluting 10.0 mL of a 5,0 M stock solution with water to a final volume of 100.0 mL The following formula is used to calculate the concentration of the standard solution. C2= V2 C1XV1 What is the value of V2? Choose... What is the value of V ? Choose... What is the value of C,? Choose... Choose... 100.0 mL 110.0 mL 10.0 mL 5.0 M Next page

Standardization of NaOH Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 D. 785 O.l690g 0. 8239 Mass of KHP Final buret 16.30mL: 14.05ML 17.10ML reading Initial buret 0,00mL 0.0vmL O.comL reading Volume of NaOH Calculate the molarity of the NaOH for each trial: Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 Calculated Molarity Average Molarity M

Part A) A 10.0 mL sample of 0.250 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0900 mol/L NaOH(aq) and then diluted to a final volume of 100. mL.Calculate the concentration of Ni2+ ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.ksp: 5.48e-16

ACID-BASE TITRATION PRELA BOUESTIONS NAME NaOH according to the following equation HC,H O2 NAOH NACH O2 НОН acid. WELBL0 2. Calculate the grams of acetic acid in one liter of the vinegar. 52.5g S. The 4.00 mL sample of vinegar had a mass of 4.056 g. Calculate the grams of vinegar in one liter. 3. 4. Calculate the % acetic acid in the vinegar. g acetic acid x 100 g vinegar % acetic acid || 95