You have two solutions of chemical A.To determine which has the highest concentration of in molarity, what the minimum number of the following you must know?
I. the mass in grams of A in each solution
II. the molar mass of A
Ill., the volume of water added to each solution
IV. the total volume of the solution
a. 3
b. 1
c. You must know all of them.
d. 0
e. 2

Answers

Answer 1

c. To determine which has the highest concentration in molarity you must know all of them.

To determine the molarity of a solution, you must know the mass in grams of A in each solution, the molar mass of A, the volume of water added to each solution, as well as the total volume of the solution.

Mass and molar mass gives you the moles of A in each solution, while the volume of water and total volume of the solution gives you the concentration of A in each solution. Therefore, you must know all four pieces of information to determine which solution has the highest concentration of A in molarity.

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Related Questions

A compound is found to contain 26.73 % phosphorus, 12.09 % nitrogen, and 61.18 % chlorine by mass. What is the molecular
formula for this compound

Answers

The Molecular formula for this compound would be [tex]N{6} Cl{12} P{6}[/tex]

What is Molecular formula?

The molecular formula is described as an expression that defines the number of atoms of each element in one molecule of a compound

The first step is to find out how many grams of each element are in one mole of the compound.

We do this because we have the molar mass of the compound, as well as the percent mass of each element.

695g * 26.73% = 186g of Phosphorous/mol of compound.

695g * 12.09% = 84g of Nitrogen/mol of compound.

695g * 61.18% = 425g of Chlorine/mol of Compound.

Because we know how many grams of each element are present per mole of compound, we can use the molar masses of each element to find out how many moles of each element are present per mole of the compound.

186g P * (1mole P/30.1g) = 6 moles of Phosphorous.

84g N * (1mole N/14g) = 6 moles of Nitrogen.

425g Cl * (1mole/35g) = 12 moles of Chlorine.

Therefore, the molecular formula for this compound would be [tex]N{6} Cl{12} P{6}[/tex]

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You are titrating a solution of sodium hydroxide of unknown concentration with 0.500 M of phosphoric acid. It required 16.4 mL of H3PO4 solution to neutralize 10.0 mL of NaOH solution. Calculate the molar concentration of sodium hydroxide solution?

Answers

A 45-mL sample of H-Cl with an unknown content was used to titrate Na-OH. One mole of phosphoric acid requires three moles of sodium hydroxide to neutralize it.

Three moles of sodium hydroxide are required for every mole of phosphoric acid. The balanced equation reveals the following: 1 mol of H3PO4 and 3 mol of NaOH react chemically. The balanced equation makes it abundantly evident that 2 moles of NaOH react with 1 mole of sulphuric acid to produce the desired products. Number of moles of solute/volume of solution in lit. = 2 moles of Na-OH are needed to thoroughly react with 1.00 mole of sulfuric acid. Therefore, 10g of Na-OH should be used to create a 500 mL 0.5 M solution.

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Using the following standard reduction potentials,
Fe3+(aq) + e- →Fe2+(aq) E° = +0.77 V
Ni2+(aq) + 2 e- →Ni(s) E° = -0.23 V
calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions.
Ni2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Ni(s)
a) E° = -1.00 V, spontaneous
b) E° = +1.00 V, nonspontaneous
c) E° = +1.00 V, spontaneous
d) E° = -1.00 V, nonspontaneous

Answers

d) E° = -1.00 V, nonspontaneous is the correct answer.

Regarding the specified chemical reaction:

[tex]Ni^{2+}(aq.) + 2Fe^{2+}(aq.)[/tex] → [tex]2Fe^{3+} (aq.) + Ni(s)[/tex]

In this case, iron is being oxidized because it is losing electrons, whereas nickel is being reduced because it is receiving electrons.

We know that:

[tex]E^{0}_{(Fe^{3+}/Fe^{2+})} = 0.77V[/tex]

[tex]E^{0}_{(Ni^{2+}/Ni)} = -0.23V[/tex]

The substance that is being oxidized acts as the cathode and the substance that is being reduced acts as the anode.

We use the equation to determine the reaction [tex]E^{0}_{cell}[/tex].

[tex]E^{0}_{cell} = E^{0}_{cathode} - E^{0}_{anode}[/tex]

[tex]E^{0}_{cell} = -0.23-0.77= -1.0 V[/tex]

The following shows how standard electrode potential and standard Gibbs free energy relate:

Δ[tex]G^{0} = -nFE^{0}_{cell}[/tex]

The standard electrode potential of the cell for the mentioned cell is negative. As a result, the reaction's standard Gibbs free energy change will become positive, making it non-spontaneous.

So, the mentioned response is non-spontaneous.

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