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3 years ago

Formula for Ni2+ and NO3

Chemistry

1 answer:

lyudmila [28]3 years ago

6 0

The formula of a compound is $Ni(NO_3)_2$

Given:

The ions $Ni^{2+}$ and $NO_3^-$

To find:

The formula for ions $Ni^{2+}$ and $NO_3^-$

Solution:

The ion with a positive charge (cation) = nickel ion = $Ni^{2+}$

The ion with a negative charge (anion) = nitrate ion = $NO_3^-$

Valency on nickel ion = 2

Valency on nitrate ion = 1

Using the criss-cross method as shown in image

The formula of a compound : $Ni(NO_3)_2$

The name of a compound is nickel(II) nitrate

$Ni^{2+}+2NO_3^-\rightarrow Ni(NO_3)_2$

The formula of a compound is $Ni(NO_3)_2$

Learn more about ions here:

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Given the balanced equation:

Marta_Voda [28]

The answer is (2) A bond is formed and energy is released. The left side of equation is I atom and the right side of equation is I2 molecule. So the bond is formed between I atom to form I2 molecule. And forming bond will release energy while breaking bond will absorb energy.

7 0

3 years ago

A potassium atom (atomic number 19) and a bromine atom (atomic number 35) can form a chemical bond through a transfer of one ele

liubo4ka [24]

Answer:

A potassium atom (atomic number 19) and a bromine atom (atomic number 35) can form a chemical bond through a transfer of one electron. The potassium ion that forms has 18 electrons. What best describes the bromide ion that forms? It is a negative ion that has one more valence electron than a neutral bromine atom.

Explanation:

7 0

2 years ago

An amphoteric salt is one that contains an anion that can act as either an acid or a base in water. Baking soda, NaHCO3, is an e

LenKa [72]

Answer:

pH = 8.34

Explanation:

The equilbriums of the amphoteric HCO₃⁻ (Ion of NaHCO₃) are:

H₂CO₃ ⇄ <em>HCO₃⁻</em> + H⁺ Ka1 <em>-Here, HCO₃⁻ is acting as a base-</em>

<em>HCO₃⁻</em>⇄ CO₃²⁻ + H⁺ Ka2 <em>-Here, is acting as an acid-</em>

Where Ka1 = 4.3x10⁻⁷ and Ka2 = 4.8x10⁻¹¹. As pKa = -log Ka:

pKa1 = 6.37; pKa2 = 10.32

As the pH of amphoteric salts is:

pH = (pKa1 + pKa2) / 2

3 0

2 years ago

49.9 ml of a 0.00292 m stock solution of a certain dye is ddiluted to 1.00 L. the diluted solution has an absorbance of 0.600. w

inna [77]

Complete Question

49.9 ml of a 0.00292 m stock solution of a certain dye is diluted to 1.00 L. the diluted solution has an absorbance of 0.600. what is the molar absorptivity coefficient of the dye

Answer:

The value is $\epsilon = 4118.1 \ M^{-1} cm^{-1}$

Explanation:

From the question we are told that

The volume of the stock solution is $V_1 = 49.9 mL = 0.0499 \ L$

The concentration of the stock solution is $C_1 = 0.00292 \ M$

The volume of the diluted solution is $V_2 = 1.00 \ L$

The absorbance is $A = 0.600$

Generally the from the titration equation we have that

$C_1 * V_1 = C_2 * V_2$

=> $0.00292 * 0.0499 = C_2 * 1$

=> $C_2 = 0.0001457 \ M$

Generally from Beer's law we have that

$A = \epsilon * l * C_2$

=> $\epsilon = \frac{A}{ l * C_2 }$

Here l is the length who value is 1 cm because the unit of molar absorptivity coefficient of the dye is $M^{-1} * cm^{-1}$

$\epsilon = \frac{0.600}{ 1 * 0.0001457 }$

=> $\epsilon = 4118.1 \ M^{-1} cm^{-1}$

4 0

2 years ago

How many molecules of H2O are there in 1.0 g of H2O?

NISA [10]

Molar mass H₂O = 18.0 g/mol

number of moles :

1.0 / 18.0 => 0.055 moles

1 mole -------------- 6.02 x 10²³ molecules
0.055 moles -------- ? molecules

molecules = 0.055 x ( 6.02 x 10²³) / 1

molecules = 3.311x10²² / 1

= 3.311 x 10²² molecules

hope this helps!

8 0

2 years ago