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please solve these questions with specific
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5) Calculate the mass of Nal necessary...
Report Questions 1. Approximately 1 mL of two clear, colorless solutions-0.1 M Ba(NO3)2and 0.1 M N...
Report Questions 1. Approximately 1 mL of two clear, colorless solutions-0.1 M Ba(NO3)2and 0.1 M Na2SO4- were combined. Upon mixing, a thick, milky white precipitate formed. After centrifugation, the solution above the precipitate was found to be clear and colorless. Based on these observations, determine if a reaction occurred. If so, write the balanced chemical equation and net ionic equation for the reaction. 2. Predict if a reaction would occur when solutions of 0.1 M Al(NO3)2and 0.1 M KI are combined. Explain...
I will fail to dissociate. E) none of the above It will do sol V Sally....
I will fail to dissociate. E) none of the above It will do sol V Sally. It will dissociate 14) If you had an aqueous mixture that contained Ag. different soli Terent solids could precipitate if a chloride solution was added A1 (B92 C) 3 D) 4 K contained Ag+, K+, and Pb2+ cations, how many AYA Kitcl > KCI) Pb²+ 200 - PbCl26) E) no solids will precipitate 3) What type of a reaction occurs when a potassium nitrate...
I really just need all the equations, please and thank you. MATERIALS: cene nitric acid, HNO,...
I really just need all the equations, please and thank you.
MATERIALS: cene nitric acid, HNO, 3.0M sodium hydroxide, NaOH 6.0 M sulfuric acid, H2SO4 zine metal DI water PROCEDURE: Make sure you record detailed observations after almost every step. You will also need to write the balanced chemical equations for almost every step. Make sure you answer any questions associated with a step 1. Weigh approximately 0.5 g of copper metal and record the weight. Place the copper in...
Solve and show work: Consider the precipitation reaction that takes place when a water solution of...
Solve and show work: Consider the precipitation reaction that takes place when a water solution of aluminum nitrate, Al(NO3)3, is added to a water solution of potassium phosphate, K3PO4. a. Write a balanced equation for this reaction. b. What is the maximum mass of aluminum phosphate that will precipitate from a solution prepared by adding an excess of an Al(NO3)3 solution to 50.00 mL of 1.525 M K3PO4?
7. In the lab one day, you mixed 30.0 mL of a 0.500 M Na:CO) solution...
7. In the lab one day, you mixed 30.0 mL of a 0.500 M Na:CO) solution with 45.0 mL of a 0.667 M Cr(N0)) solution. Write a balanced chemical equation complete with physical states: a. Write the ionic equation for the reaction: b. ENG 2 C- CraCoo) c. Write the net-ionic equation for the reaction: 2 C Calculate the mass of the precipitate formed (hint: find the limiting reactant) d. Calculate the molarities of ions remaining in solution after the...
i dont know what im doing. help. 4.3-Precipitation Reactions 3. The following molecular views show reactant...
i
dont know what im doing. help.
4.3-Precipitation Reactions 3. The following molecular views show reactant solutions for a precipitation reaction (with H,O molecules omitted for clarity). a) Which compound is dissolved in beaker A: KCI, Na2SO4, MgBrz, or Ag2SO.? b) Which compound is dissolved in beaker B: NH,NO3, MgSO Ba(NO3), or CaFZ? c) Write a balanced molecular, total ionic, and net ionic equations for the reaction that occurs when solutions A and B are mixed. d) If 1 L...
A 829.0-mL aliquot of 0.880 M aqueous potassium hydroxide is mixed with 829.0 mL of 0.880...
A 829.0-mL aliquot of 0.880 M aqueous potassium hydroxide is mixed with 829.0 mL of 0.880 M aqueous magnesium nitrate. ( just need d.) a.)Write a balanced chemical equation for any reaction that occurs. b.) The precipitate is magnesium hydroxide Mg(OH)2 c.) What mass of precipitate is produced? d.)Calculate the concentration of each ion remaining in solution after precipitation is complete. Assume that the precipitate is completely insoluble The concentration of K+ = ____ M The concentration of OH- =...
1. When 0.100 L of a solution containing 0.15 M KBr is added to 0.100 L...
1. When 0.100 L of a solution containing 0.15 M KBr is added to 0.100 L of a solution containing 0.15 M Pb(NO3)2, what precipitate will form? PbBr2 PbBr Pb(NO3)2 KNO3 K(NO3)2 PbK KBr 2. What is the driving force for the reaction described in Q1 above? The formation of a new insoluble ionic compound The formation of a gas the formation of water molecules the formation of new ions the formation of a new soluble ionic compound 3. Write...
6) (50 pnts) You make two 150. mL solutions (density of water is 0.999 g/mL). One...
6) (50 pnts) You make two 150. mL solutions (density of water is 0.999 g/mL). One is a solution made from 2.05 g of ammonium chloride and the other from 12.7 g of lead(II) nitrate. You mix the two solutions together yielding a yellow precipitate. a) Write the molecular equation for the above reaction: b) Write the complete ionic equation for the above reaction: c) Write the net ionic equation for the above reaction: d) What mass of solid is...
You could do only one if you want, any help would be appreciated. 41. What mass...
You could do only one if you want, any help would be
appreciated.
41. What mass of solid aluminum hydröxide call be produced when 50.0 mL of 0.200 M AI(NO3)3 is added to 200.0 mL of 0.100 M KOH? 42. What mass of barium sulfate can be produced when 100.0 mL of a 0.100 M solution of barium chloride is mixed with 100.0 mL of a O.100 M solution of iron(III) sulfate? 43. How many grams of silver chloride can...
I will fail to dissociate. E) none of the above It will do sol V Sally. It will dissociate 14) If you had an aqueous mixture that contained Ag. different soli Terent solids could precipitate if a chloride solution was added A1 (B92 C) 3 D) 4 K contained Ag+, K+, and Pb2+ cations, how many AYA Kitcl > KCI) Pb²+ 200 - PbCl26) E) no solids will precipitate 3) What type of a reaction occurs when a potassium nitrate...
I really just need all the equations, please and thank you.
MATERIALS: cene nitric acid, HNO, 3.0M sodium hydroxide, NaOH 6.0 M sulfuric acid, H2SO4 zine metal DI water PROCEDURE: Make sure you record detailed observations after almost every step. You will also need to write the balanced chemical equations for almost every step. Make sure you answer any questions associated with a step 1. Weigh approximately 0.5 g of copper metal and record the weight. Place the copper in...
7. In the lab one day, you mixed 30.0 mL of a 0.500 M Na:CO) solution with 45.0 mL of a 0.667 M Cr(N0)) solution. Write a balanced chemical equation complete with physical states: a. Write the ionic equation for the reaction: b. ENG 2 C- CraCoo) c. Write the net-ionic equation for the reaction: 2 C Calculate the mass of the precipitate formed (hint: find the limiting reactant) d. Calculate the molarities of ions remaining in solution after the...
i
dont know what im doing. help.
4.3-Precipitation Reactions 3. The following molecular views show reactant solutions for a precipitation reaction (with H,O molecules omitted for clarity). a) Which compound is dissolved in beaker A: KCI, Na2SO4, MgBrz, or Ag2SO.? b) Which compound is dissolved in beaker B: NH,NO3, MgSO Ba(NO3), or CaFZ? c) Write a balanced molecular, total ionic, and net ionic equations for the reaction that occurs when solutions A and B are mixed. d) If 1 L...
6) (50 pnts) You make two 150. mL solutions (density of water is 0.999 g/mL). One is a solution made from 2.05 g of ammonium chloride and the other from 12.7 g of lead(II) nitrate. You mix the two solutions together yielding a yellow precipitate. a) Write the molecular equation for the above reaction: b) Write the complete ionic equation for the above reaction: c) Write the net ionic equation for the above reaction: d) What mass of solid is...
You could do only one if you want, any help would be
appreciated.
41. What mass of solid aluminum hydröxide call be produced when 50.0 mL of 0.200 M AI(NO3)3 is added to 200.0 mL of 0.100 M KOH? 42. What mass of barium sulfate can be produced when 100.0 mL of a 0.100 M solution of barium chloride is mixed with 100.0 mL of a O.100 M solution of iron(III) sulfate? 43. How many grams of silver chloride can...
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