Answer:
a.reducing agent reduces other elements and make itself oxidized
b.Oxidizing agent reduces itself and make other element oxidized
c.Oxidation state is apparent charge on an atom
Explanation:
The water dissolves the salt because the water molecules are able to interact with the salt-forming particles, called ions. When the water Interacts with the trainers of the salt ions, the solid salt crystal structure Suffers breakdown, until the trainers of the salt ions are completely surrounded by water molecules. At this time the salt is fully dissolved by water.
hope this helps!
Your limiting is CuCI2 and the excess is KI (from what i’ve heard from my tc to find it just use the moles or look at the grams)Do you want me to do the qn and give u the ans or?
Explanation:You have more grams of KI than CuCI2
irl example : I need 200g of flour to bake 1 muffin and 100g of butter.But I have 300g of butter and only 200g of flour.This means I can only bake up to 1 muffin since I got excess grams of butter.But to use up all my 300g of butter I need 400g more of flour.Making my butter the excess while my flour the limiting since I have less of it and it also determines how much muffin would I get at the end of the bake.
im sorry if that example sounds clowny T-T
Molarity of Ag+ is less than the molar solubility thus ppt will not occur.
Balanced reaction-:
<h3>2AgNO3(aq)+K2CrO4(aq)→Ag2CrO4(s)+2KNO3(aq)</h3>
Moles of AgNO3=mass(g)molar mass (g/mol) =2.7×10−5g / 169.86 gmol
=1.589⋅10^−7 mol
Molarity of Ag+=moles of solute(L)=1.589⋅10−7 mol0.015 L=1.059⋅10−5M
Ksp of Ag2CrO4
=[Ag+]2[CrO42−]
1.2⋅10−12=[2s]2[s]
4s3=1.2⋅10−12
s=6.69⋅10−5 M
Molarity of Ag+ is less than the molar solubility thus ppt will not occur.
<h3>What is the molarity calculation formula?</h3>
The volume of solvent required to dissolve the provided solute is multiplied by the ratio of the moles of the solute whose molarity has to be computed. (M=frac{n}{V}) The molality of the solution that needs to be computed in this case is M. n is the solute's molecular weight in moles.
Learn more about Molarity:
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