Watch the Introductory Video and Support Information on the upper left to learn how touse this virtual lab.i.i.Place a bottle of 0.1 M NaCl solution, the unknown AgNO, solution, a 250 mL Erlenmeyerflask, a 10 mL pipette, and a burette (in Glassware→Other) on the workbench. If thebench is said to be too full, set the items along the right side the bench to save space.Record the volume of the original unknown AGNO, solution in the Data sheet.Workbench 1Unknown AgNO,52.500 ml 25.0c0.1MNaCI100 00 ml 25.OC250 ml Flask0.0000 ml 25.0c10 ml Pipette00000 m25.0C50 ml Burette0.0000 ml25.0cii.Transfer 50 mL of 0.1 M NaCl solution into the burette.iv.Withdraw 10 mL of the unknown AGNO, solution into the pipette and transfer the solutioninto the empty Erlenmeyer flask.v.Deliver 1 mL of the 0.1 M NaCl solution from the burette into the 10 mL unknown AgNO,solution. Pay attention to mass of AgCl displayed in the information windowInformationName 250 m FlaskVolume 11.007 mlSpecies (s)ams10 Poette00000 5onown AgNO,s0025.0CTemperature 2500cPrecisept 700From 50 m. Burete to 20 m Fa1.00 m transtemed250m Flak11007250c0IMNCso000 250cRepeat addition of 1 mL of the 0.1 M NaCl solution from the burette into the unknownsolution until the mass of AgCI doesn't change any more. Record the mass of theprecipitate AgCI on the Data Sheet.vi. Volume of the original unknown AgNO3 solution =mLMass of AgCI (s) =Mole of AgCl =(mole = mass /molar mass)Calculate mole of AGNO, in the 10 mL unknown solution based on the following reactionequation:NaCla) + AgNOs(aq)- NANO(aq) + AgCl)Mole of AgNO3 in the 10 mL unknown solution =use the coefficient ratio)_(hint,

Answered: Image /qna-images/answer/87c167e0-d90d-4a1e-9c69-fe40062f14e8.jpg

Volume of the original unknown AgNO3 solution = mL Mass of AGCI (s) = Mole of AgCI = (mole = mass Imolar mass) Calculate mole of AGNO, in the 10 mL unknown solution based on the following reaction equation: NaClag) + AGNO3(aq) → NANO3(ag) + AgCla) Mole of AgNO3 in the 10 mL unknown solution = use the coefficient ratio) _(hint,

Volume of the original unknown AgNO3 solution = mL Mass of AGCI (s) = Mole of AgCI = (mole = mass Imolar mass) Calculate mole of AGNO, in the 10 mL unknown solution based on the following reaction equation: NaClag) + AGNO3(aq) → NANO3(ag) + AgCla) Mole of AgNO3 in the 10 mL unknown solution = use the coefficient ratio) _(hint,

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. Write the net ionic equation for the following molecular equation. MgSO4(aq) + Na₂CO3(aq) MgCO3(s) + Na₂SO4(aq) + +
If 2.00 grams of an unknown DIPROTIC acid (H2A) is titrated with 34.0 mL of 1.35 M NaOH, what is the molar mass (g/mol) of the diprotic acid? H2A+2NaOH⟶2H2O+Na2AH2A+2NaOH⟶2H2O+Na2A (Hint: See equation below in which mm is molar mass (units: g/mol), m is mass (unit: g), and mol isnumber of moles (unit: mol)). mmacid=macidmolacidmmacid=macidmolacid Molar Mass = ___________ g/mol (input the numeric value only!) Remember: use correct significant figure rules. Significant figures always matter in Chemistry!
Consider the reaction below: 6 ABCIO 3(aq) + 1 Al2S3{aq) 3 Ag2Sts) + 2 Al(CIO3]a{a} (OR "6" A gCI O3la q) + "1" A I½S3(a q) right arrow "3" Ag,S + "2" A I(CI Ota a) The sum of the coefficients of the full ionic equation is
The dilution equation, rearranged to solve for ?1 is ?1=?2?2?1 where ?1 and ?1 are the initial concentration and volume, respectively, and ?2 and ?2 represent the final concentration and volume, respectively. A student needs to prepare 50.0 mL of 1.10 M aqueous H2O2 solution from 4.8 M H2O2 stock solution. Set up an equation to solve for the volume of stock solution needed by plugging the given values into the equation.
See image below....
4. Calculate the calculate the mass of precipitate formed from 5.0 g of strontium chloride. Li3PO4(aq) → Sr3(PO4)2(S) + LiCl(aq) _SrCl₂(aq) + 5. What mass of aluminum hydroxide in needed to neutralize 5.00 g of hydrochloric acid? Al(OH)3(s) + _HCl(aq) → ___AlCl3(aq) + _H₂O(1) 195
A reaction is carried out by mixing together a solution of HF and a solution of NaOH. HF (aq) + NaOн (аq) —> н,О (1) Assume the purple particles below each represent 1 mole of particles. Construct the balanced net ionic equation by dragging the purple components into the gray boxes. Drag each unreacted spectator ion along with its balancing coefficient into the blue box that represents the aqueous solution. Remember when you identify spectator ions to look carefully at what changes chemically! + NaF (aq)
Fe(s) + CuSO4(aq) and KCL(aq) + AgNO3(aq) For each one write total and net ionic equations.
The initial concentration of oxalic acid is 0.315 M and for KMnO4 is 0.0113 M. What is the concentration of oxalic acid remaining when the limiting reactant has completely reacted? Thanks.
101 Chem101 G Balance the following chemical b My Questions | bartleby X + app.101edu.co E Apps M Gmail YouTube Мaps VitalSource Books... Question 16 of 24 Submit Balance the following chemical equation (if necessary): Na*(aq) + CI (aq) + Ag*(aq) + NO: (aq) → Na*(aq) + AgCI(s) + NO: (aq) |4– D2+ N3+ 4+ 1 2 3 4 6. 7 8 9 04 (s) (1) (g) (aq) CI Ag NO Na Cr Ar fishes lab.pdf Early Chrodates La...pdf Show all PDF PDF ... 2.
Identify the spectator ions in the following molecular equation. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq) K+ and Br Ag+ and Br Ag+ and NO3 OK* and NO3 O There are no spectator ions in this reaction.