of 15 > Tin(IV) sulfide, SnS₂, a yellow pigment, can be produced using the following reaction. SnBr(aq) + 2 Na, S(aq) →→→ 4 NaBr(aq) + SnS₂ (s) - Suppose a student adds 39.8 mL of a 0.562 M solution of SnBr4 to 50.2 mL of a 0.151 M solution of Na, S. Identify the limiting reactant. SnBr4 O Na₂S O NaBr O SnS₂ Calculate the theoretical yield of SnS₂. theoretical yield: The student recovers 0.396 g of SnS₂. Calculate the percent yield of SnS, that the student obtained.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Given :
SnBr4 (aq) + 2 Na2S(aq) → 4 NaBr(aq) + SnS₂(s)
Experimental yield = 0.396 gram
39.8 mL of a 0.562 M solution of SnBr4
50.2 mL of a 0.151 M solution of Na2S
Needed information : molar mass of SnS2 = 182.84 g/mol
To find :
Identification of limiting reactant ,theoretical yield and percentage yield
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