Copper II Lab

Limestone consists mainly of the mineral calcite, CaCO3.  The carbonate content of 0.5143 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel the CO2: CaCO3(s)  +  2H+  ⟶⟶ Ca2+  +  CO2↑↑ +  H2O The excess acid requied 39.96 mL of 0.1004 M NaOH for complete titration: OH-   +   H+  ⟶⟶ H2O Find the weight percent of calcite in the limestone.

5mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl) The Kb for ammonia is 1.75 x 10-5  1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a balanced chemical equation for the equilibrium of ammonia in water. 2) What is the pH of the ammonia solution prior to the addition of any HCl?

Molarity of titrant (NaOH):  0.4550 M   Trial # First Second Third Fourth Initial buret reading 0.15 mL 2.43 mL 1.32 mL 0.58 mL Final buret reading 18.62 mL 20.87 mL 20.03 mL 19.14 mL Volume of titrant used 18.47 mL 18.44 mL 18.71 mL 18.56 mL               Write the balanced neutralization reaction that occurs when you titrate the acetic acid (HC2H3O2)  with sodium hydroxide (NaOH). Hint: It’s in the background. HC2H3O2 (aq) + NaOH (aq) → NaC2H3O2 (aq) + H2O (l)   Using data from all 4 titrations, calculate the average volume of standard NaOH solution required to titrate 10.00 mL of the vinegar solution (Show your work).     Average volume to titrate 18.47+18.44+18.71+18.56/4=   Average Volume = 18.545  mL   Calculate the average number of moles of NaOH used in the titrations (show your work).     Average Moles NaOH =              moles   Calculate or determine (give reasoning) the number of moles of acetic acid in the 10.00 mL…

Fill out the tables and find pH

What are the Initial Concentrations of Fe3+ and SCN-? Fe3+ (aq) + SCN– (aq) à FeSCN2+ (aq) Flask # 0.2 M Fe(NO3)3 in 0.50M HNO3 0.50M HNO3 2.00 x 10–3 M KSCN in 0.50M HNO3 Initial [Fe3+] Initial [SCN-] Initial [FeSCN2+] Blank 5 mL 5 mL 0 mL       1 5 mL 4 mL 1 mL       2 5 mL 3 mL 2 mL       3 5 mL 2 mL 3 mL       4 5 mL 1 mL 4 mL       5 5 mL 0 mL 5 mL       Show a sample dilution calculation for flask 1. Hint: M1V1 = V2V2

based on the data tables provided, what is % CH3COOH in vinegar

For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K, data in the ALEKS Data tab. Does solubility change with pH? highest solubility compound pH = 4 pH = 6 pH = 7 yes CaCl, O no O yes AGCN no O yes PbF, no ?

A student was titrating a solution of hydrazine, H₂NNH2, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 1 NEXT 40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 80 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base.. Before (mol) Change (mol) After (mol) 6.00 × 10³ -6.00 × 10³ 0 Initial (M) Change (M) Equilibrium (M) 0.100 + x 0 H₂NNH₂(aq) 0.100 7.00 x 10" 0.100 - x H₂NNH3*(aq) + Question 8 of 23 2 0.100 0.200 + x 0.200 -7.00 x 10³ + 0.200 A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by…

For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 5 pH = 4 pH = 3 Ca, (PO.), yes O no O yes AgCN O no yes PbCl2 no Explanation Check Accessibili O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy 17 MacBook Air F10 F9 F7 F8 o oo o

Only typed solution

A student titrates a 35.00 mL sample of 0.0100 M sodium hypochlorite (NaClO), a salt containing the conjugate base of hypochlorous acid (HClO, Ka = 3.0 x 10-8), with 0.0125 M HCl.?????(??) + ???(??) → ????(??) + ????(??)Determine the pH of the solution after 30.00 mL of HCl has been added.

3a) A student determines the concentration of a sodium hydroxide solution by titration with standardized KHP. S/he obtains the values: 0.190 M, 0.202 M, and 0.205 M. Should the value 0.190 M be rejected? Apply the Q Test. For three values Q must be greater than 0.94 to reject the number. Q = suspect nearest | largest - - smallest b) The student de to repeat the experiment two more The five values now include: 0.190 M, 0.202 M, 0.205 M, 0.201M and 0.203M. Use the Q Test to see if the first value may be rejected. For five values Q must be greater than 0.64 to reject the number. c) Solve for the average Molarity of the measurements from part b with and without the rejected number. Is there value in repeating an experiment several times?

o ooo For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 2 pH = 3 pH = 5 yes PbCl2 O no dla O yes BaCO, O no O yes ZnS O no Explanation Check 2021 McGraw Hill Education All Rights Rese Terms of Use Privacy Accessibility O VI 1:41

For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility highest solubility compound change with pH? pH = 4 pH = 6 pH = 7 NaBr yes no Ca, (PO4)2 Ca(OH)2 yes no yes no ☑ ? 000 18 Ar

For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'lIl find K, data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 5 pH = 4 pH = 2 O yes CaCO, O no O yes CuBr O no O yes Ni(OH), O no

Would the calculated value of the molarity of the NaOH solution be too high or too low or unchanged if the flask into which the student weighed the KHP was wet? Unchaged. The NaOH concentration wouldn't be affected by the amount of water. Too high. The NaOH solution is diluted by the water Too low. The NaOH solution is diluted by the water.

A titration analysis of a 345.0 mL aqueous HBr solution was performed and the endpoint was reached upon the addition of 191.05 mL of 2.815 M aqueous KOH solution. What is the concentration (in M) of the HBr solution? HBr(aq) + KOH(aq) ——> KBr(aq) + H2O(l)

Part A: Standardization of a Sodium Hydroxide Solution   Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml   Calculations   Titration 1 Titration 2 Titration 3 Moles of KHP       Moles of NaOH       Molarity of NaOH         Average Molarity of NaOH: _______________

22.5 mL of an HNO3 solution were titrated with 31.27 mL of a 0.167 M Ca(OH)2 solution to reach the equivalence point. What is the molarity of the HNO3 solution? 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H₂O [?]M Hint: Did you account for the mole ratio? Molarity (mol/L) -2023 International Academy of Science. All Rights Reserved. Q Search DELL Enter