BaCO3, which will precipitate out
Result is Nacl and BaCo3
A red blood cell is placed into each of the following solutions. Indicate whether crenation, hemolysis, or neither will occur. Solution A: 3.21% (m/v) NaCl Solution B: 1.65% (m/v) glucose Solution C: distilled H2O Solution D: 6.97% (m/v) glucose Solution
A 0.100 M solution of K2SO4 would contain the same total ion concentration as which of the following solutions? A. 0.0800 M Na2CO3 B. 0.100 M NaCl C. 0.0750 M Na3PO4 D. 0.0500 M NaOH
Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states. A. nitric acid, HNO3 , and calcium hydroxide, Ca(OH)2 B. lead(II) nitrate, Pb(NO3)2 , and potassium iodide, KI
When an aqueous solution suspected of containing Ba2+ or Pb2+ or both are mixed with sulfuric acid a precipitate forms. in another test, when the original solution is mixed with an aqueous solution of sodium sulfide no precipitate forms. What do these two
1) Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct? A) Both KNO3 and NH4SO4 precipitate from solution B) A gas is released C) NH4SO4 will precipitate from solution D) KNO3 will precipitate from
What is the precipitation of CaSO4 and Na2CO3 when mixed? What is the net ionic equation?
What is the finaly concentration of barium ions, Ba2+, in soulution with 100 ml of .1 M BaCl2 is mixed with 100ml of .05M H2SO4?
predict which three of the following five aqueous solutions should react with solid aluminum metal (the elemental form of aluminum): AgNO3, Na2CO3, CuSO4, CaCl2, Pb(NO3)2
what products result from mixing aqueous solutions Cu(C2H3O2)2(aq) and Rb3PO4(aq)?
When aqueous solutions of sodium sulfate and lead (II) nitrate are mixed lead sulfate precipitates out of soultion. Calculate the mass of lead (II) sulfate that should form when 1.25 L of 0.0500 M Pb(NO3)2 and 2.00 L of 0.0250 M Na2SO4 are reacted
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NOREACTION. Are my answers below correct? I used the textbook 1. sodium chloride and lead (II) acetate
Use the unbalanced chemical equation to answer the question. 2NaHCO3 → Na2CO3 + CO2 Which of the following can be added to the products to balance the equation? H^2O H^2 O^2 CH^2OH
will a red blood cell undergo crenation, hemolysis, or no change in each of the following solutions? 1% (m/v) glucose 2% (m/v) NaCl 5% (m/v) NaCl .1% (m/v)NaCl
Aqueous solutions of sodium sulfide and silver nitrate are mixed to form solid silver sulfide and aqueous sodium nitrate. The complete ionic equation contains which one of the following terms (when balanced in standard form)?
Calculate the theoretical yield of NaCl (using mass-to-mass calculation). (Use the mass of sodium carbonate reactant used as the starting point, along with the relevant mole ratio from the balanced equation to perform this calculation). Work must be shown
Arrange the following aqueous solutions in order of decreasing freezing points (lowest to highest temperature): 0.10 m Na3PO4, 0.35 m NaCl, 0.20 m MgCl, 0.15 m C6H12O6 and 0.15 m CH3COOH.
A 2.559 9 pellet containing NaCl and KCl is dissolved in water. A silver nitrate solution is mixed with water containing the pellet, and a precipitate forms. The precipitate is separated and dried and found to have a mass of 5.112 9. What is the percent
Which of the following pairs of aqueous solutions will react when mixed? K2CO3 + HNO3 HCl + LiOH MgCl2 + KOH Li2S + HCl All of these solution pairs will produce reactions.
How much Na2CO3 would you weigh to prepare M/20 Na2CO3 solution in 100cm3 volumetric flask?
a 5.95 g sample of AgNO3 is reacted with excess BaCl2 according to the equation 2AgNO3 + BaCl2 yields 2AgCl + Ba(NO3)2 to give 3.17 g of AgCl. What is the percent yield of AgCl?
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