Q3: A: What mass of AgNO3 is needed to convert 3.46g of Na2CO3 to Ag2CO3, and calculatethe mass of A92CO3 will be formed? Discuss your results.2AGNO3(aq) +Na2CO3(aq) → Ag2CO3(e) + 2NaNo3(aq)B: Calculate the Normality of solutions containing the following with discussing yourresults:-1) 8 gm /L of Na2CO3 (when the CO3² reacts with two protons).2) 9.5 gm /L of K2CR2O7 (the Cr is reduced to Cr*3).

A. 1 mole of sodium carbonate reacts with 2 moles of silver nitrate 105.98 g of sodium…

Q3: A: What mass of AgNO3 is needed to convert 3.46g of NażCO3 to Ag2CO3, and calculate the mass of A92CO3 will be formed? Discuss your results. 2AGNO3(aq) +N22CO3(a9) → Ag:CO3(9) + 2NAN03(aq) B: Calculate the Normality of solutions containing the following with discussing your results:- 1) 8 gm /L of N22CO3 (when the CO3? reacts with two protons). 2) 9.5 gm /L of K2Cr2O7 (the Cr is reduced to Cr*³).

Q3: A: What mass of AgNO3 is needed to convert 3.46g of NażCO3 to Ag2CO3, and calculate the mass of A92CO3 will be formed? Discuss your results. 2AGNO3(aq) +N22CO3(a9) → Ag:CO3(9) + 2NAN03(aq) B: Calculate the Normality of solutions containing the following with discussing your results:- 1) 8 gm /L of N22CO3 (when the CO3? reacts with two protons). 2) 9.5 gm /L of K2Cr2O7 (the Cr is reduced to Cr*³).

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

An experimenter reacts 30.0 mL of a BaCl2 solution with excess AgNO3 as shown in the unbalanced equation below. If 2.58 grams of AgCl are obtained, what is the molarity of BaCl2solution? Hint: First balance the chemical equation. BaCl2 (aq) + AgNO3 (aq) ---> Ba(NO3)2 (aq) + AgCl (s)
Consider the reaction: 2 NaBH4(aq) + H₂SO4(aq) → 2 H₂(g) + Na₂SO4(aq) + B₂H6(9) What volume, in mL, of a 0.529 M solution of NaBH4 is required to produce 0.591 g of B₂H6? H₂SO4 is present in excess. mL Submit The desired mass of the product, B₂H6, is 0.591 g. What is this amount of B₂H5, in units of moles? mol B₂H6 Submit
10. Citric acid/citrate buffer is a pH buffer that is used for baby locations. A pH buffer is prepared by dissolving 10.85 grams C6H5O7Na2 and 11.74 grams of C6H4O7Na3 in enough water to make 250.0 mL solution. 3+ C6H50 (aq) + H₂O(1) C6H40 (aq) + H₂O* (1) The 3rd acid dissociation constant of citric acid is 4.012×10-7. Please answer the following questions. A. B. C. What is the pH of the solution? pH = Please provider your answer below. 0 00 ← $ Check answer If you add 5.000 mL, 0.5666 M of HCl to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. pH = Please provider your answer below. ← $ Check answer If you add 5.000 mL, 0.5666 M of Ba(OH)2 to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. pH =
What’s the answer in g
3. If 30.65 mL of Ca(OH), solution is needed to react with 0.240 g of primary standard H,C,0, •2H,O, what is the molarity of the Ca(OH) , solution? Са(ОН), (аq) + H,C,04 · 2H,0 (s) → CaC204 (s) + H20 (1)
Write the net ionic equation, including phases that corresponds to the reaction Cu(ClO4)2(aq) + K2CO3(aq) yields to CuCO3(s) + 2KClO4(aq)
0.529 47.629 1. Initial mass of copper 2. Mass of copper and evaporating dish 3. Mass of evaporating dish 4. Mass of recovered copper 5. Percent yield (show cafcuntions) 6. Describe the reaction Cu(s)+HNO3(aq)→. 7. Describe the reaction Cu(NO3)2(aq)+NaOH(aq)→. 8. Describe the reaction Cu(OH)2(s)-A. 9. What are you removing by this washing? 10. What copper compound is present in the beaker? 11. Describe the reaction CuSO4(aq)+Zn(s) or CuSO4(aq)+ AI(s). 12. What is present in solution? 13. What is the gas? 14. How do you know? 15. What are you removing by washing? 16. What color is your copper sample? 17. Is it uniform in appearance? 18. Suggest possible sources of error in this experiment.
When a solution of magnesium nitrate is mixed with a solution of sodium phosphate, the solid that forms is magnesium phosphate. Select the equation that represents the complete ionic equation. 17. А. Mg(NO3)2(aq) + Na,PO,(aq) → MGPO4(s) + NaNO;(aq) В. Mg2"(aq) + PO,-(aq) > MGPO,(s) С. 3Mg(NO3)2(aq) + 2Na;PO4(aq) → Mg;(PO4)2(s) + 6NANO3(aq) 3MG2"(aq) + 2PO (aq) > Mg3(PO4)2(s) 3MG2"(aq)+6NO; (ag) + 6Na"(aq) + 2PO,*(aq) →Mg;(PO4)2(s)+6NO;(aq)+ 6Na*(aq) D. Е.
b. 3H2SO4(aq) + 2Al(OH);(aq) → Al2(SO4)3(aq) + 6H2O(1) 4. In each of the following, identify the reactant that is oxidized and the reactant that is red a. 2Li(s) + F2(g) → 2LİF(s) b. Cl2(g) + 2KI(aq) → I2(s) + 2KCI(aq) atoms of H 5. Calculate each of the following a. number of Li atoms in 4.5 moles ofLi. b. moles of Cu in 7.8 x 10²1 atoms of Cu. c. moles of C2H6 in 3.75 x 1023 molecules of C2H6.
15. If 23.0 mL of a 1.00 M Ba(NO3)2 solution was reacted with 55.0 mL of a 0.700 M solution of K3PO4 to produce the solid Ba3(PO4)2 by the balanced chemical equation 3 Ba(NO3)2 (aq) + 2 K3PO4(aq) – Ba3(PO4)2(s) + 6 KNO3(aq) a. What is the limiting reagent? AS b. How many grams of Ba3(PO4)2 will be produced? elomibt.ESE -3HA
The ethyl mercaptan (C2H5SH, 62.13 g/mol) concentration in a mixture was determined by shaking a 1.534 g sample with 50.0 mL of 0.01293 M I2 in a tightly stoppered flask: 2 C2H5SH (aq) + I2 (aq) --> C4H10S2 (aq) + 2 I- (aq) + 2 H+ (aq) The excess I2 was back-titrated with 15.72 mL of 0.01425 M Na2S2O3: I2 (aq) + 2 S2O32- (aq) --> 2 I- (aq) + S4O62- (aq) Calculate the percentage of ethyl mercaptan in the sample (3 sf)
9. What is the molarity (M) of a solution if 500 mL of the solution contains 40.85 g of NaHCO₁? 10. If 42.50 mL of a 1.100 M MgCl solution is needed to completely react with 45.0 mL of AgNO, solution, what is the molarity of the AgNO, solution? Hint: use example in Section 9.5 MgCl +2AgNO 2(aq) 3(aq) 2AgCl + Mg(NO3)2(aq) (s) 4