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3 years ago

As 1 g of sodium hydroxide dissolves in 100g of water, the conductivity of the water:

2 answers:

8 0

I think the correct answer would be to increase. As salt is being dissolved in water, it dissociates into corresponding ions which would make conductivity of the solution more higher than pure water since charge particles are already present. Hope this helps.

kirill115 [55]3 years ago

4 0

Answer:

The conductivity of the resulting solution will increase.

Explanation:

The conductivity of the solution obtained by adding sodium hydroxide in water will increase as compared to pure water due to complete dissociation of sodium hydroxide into sodium ion and hydroxide ions. The conductivity increases on increase in number of ions in a solution.

The conductivity depends upon

a) number of ions

b) mobility of ion.

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Why do atoms become anion and cations (remember the octet rule and how 8 is a very important number)?

Kryger [21]

Answer:

The atoms become cations because they have lost electrons and the atoms and has a positive charge then atoms become a ions because they have gained electrons from cations and has a negative charge

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3 years ago

The lowest possible concentration of free hydrogen ions is represented by a ph value of

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3 years ago

Explain why you get a basic solution when you dissolve NaF in water.

SashulF [63]

Answer:

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3 years ago

Can someone answer this question? It's not that long

Kitty [74]

Answer:

sections 2 and 3

Explanation:

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2 years ago

On the basis of the Ksp values below, what is the order of the solubility from least soluble to most soluble for these compounds

Viktor [21]

Answer:

The order of solubility is AgBr < Ag₂CO₃ < AgCl

Explanation:

The solubility constant give us the molar solubilty of ionic compounds. In general for a compound AB the ksp will be given by:

Ksp = (A) (B) where A and B are the molar solubilities = s² (for compounds with 1:1 ratio).

It follows then that the higher the value of Ksp the greater solubilty of the compound if we are comparing compounds with the same ionic ratios:

Comparing AgBr: Ksp = 5.4 x 10⁻¹³ with AgCl: Ksp = 1.8 x 10⁻¹⁰, AgCl will be more soluble.

Comparing Ag2CO3: Ksp = 8.0 x 10⁻¹² with AgCl Ksp = AgCl: Ksp = 1.8 x 10⁻¹⁰ we have the complication of the ratio of ions 2:1 in Ag2CO3, so the answer is not obvious. But since we know that

Ag2CO3 ⇄ 2 Ag⁺ + CO₃²₋

Ksp Ag2CO3 = 2s x s = 2 s² = 8.0 x 10-12

s = 4 x 10⁻12 ∴ s= 2 x 10⁻⁶

And for AgCl

AgCl ⇄ Ag⁺ + Cl⁻

Ksp = s² = 1.8 x 10⁻¹⁰ ∴ s = √ 1.8 x 10⁻¹⁰ = 1.3 x 10⁻⁵

Therefore, AgCl is more soluble than Ag₂CO₃

The order of solubility is AgBr < Ag₂CO₃ < AgCl

8 0

3 years ago

Read 2 more answers