Unwanted elements are removed from metals by a process called

The following chemical reaction takes place in aqueous solution: AgF (aq)+ NH4Cl (aq) →AgCl(s)+ NH4F(aq) Write the net ionic equ

Nadusha1986 [10]

Answer:

The net ionic equation is: Ag⁺ (aq) + Cl ⁻ (aq) → AgCl (s)

Explanation:

1) Start by writing the total ionic equation:

The total ionic equation shows each aqueous substance in its ionized form, while the solid or liquid substances are shown with their chemical formula.

These are the ionic species:

AgF (aq) → Ag⁺ (aq) + F⁻ (aq)

NH₄Cl (aq) → NH₄⁺ (aq) + Cl ⁻ (aq)

NH₄F(aq) → NH₄⁺ (aq) + F⁻ (aq)

Then, replace each chemical formula in the chemical equation by those ionic forms:

Ag⁺ (aq) + F⁻ (aq) + NH₄⁺ (aq) + Cl ⁻ (aq) → AgCl (s) + NH₄⁺ (aq) + F⁻ (aq)

That is the total ionic equation.

2) Spectator ions:

The ions that appear in both the reactant side and the product side are considered spectator ions (they do not change), and so they are canceled.

In our total ionic equation they are F⁻ (aq) and NH₄⁺ (aq).

After canceling them, you get the net ionic equation:

3) Net ionic equation:

Ag⁺ (aq) + Cl ⁻ (aq) → AgCl (s) ← answer

4 0

3 years ago

Which synthetic polymer is made into fibers that do not wear out easily?

Alekssandra [29.7K]

C its Nylon that's the Synthetic polymer that doesnt wear out easily

6 0

3 years ago

Read 2 more answers

A volume of 500.0 mL of 0.160 M NaOH is added to 585 mL of 0.200 M weak acid ( K a = 1.28 × 10 − 5 ) . What is the pH of the res

Hitman42 [59]

Answer : The pH of the resulting buffer is, 5.22

Explanation : Given,

$K_a=1.28\times 10^{-5}$

First we have to calculate the moles of $NaOH\text{ and }HA$

$\text{Moles of }NaOH=\text{Concentration of }NaOH\times \text{Volume of solution}}=0.160M\times 0.500L=0.08mol$

and,

$\text{Moles of }HA=\text{Concentration of }HA\times \text{Volume of solution}}=0.200M\times 0.585L=0.117mol$

The balanced chemical reaction is:

$HA+(aq)+OH^-(aq)\rightarrow H_2O(l)+A^-(aq)$

Moles of HA left = 0.117 mol - 0.08 mol = 0.037 mol

Moles of $A^-$ = 0.08 mol

The expression used for the calculation of $pK_a$ is,

$pK_a=-\log (K_a)$

Now put the value of $K_a$ in this expression, we get:

$pK_a=-\log (1.28\times 10^{-5})$

$pK_a=5-\log (1.28)$

$pK_a=4.89$

Now we have to calculate the pH of buffer.

Using Henderson Hesselbach equation :

$pH=pK_a+\log \frac{[Salt]}{[Acid]}$

$pH=pK_a+\log \frac{[A^-]}{[HA]}$

Now put all the given values in this expression, we get:

$pH=4.89+\log (\frac{0.08}{0.037})$

$pH=5.22$

Thus, the pH of the resulting buffer is, 5.22

5 0

3 years ago

There are many lewis structures you could draw for sulfuric acid, h2so4 (each h is bonded to an o). part a what lewis structure(

erica [24]

Structure 1 is satisfying octet rule because each atom surrounded by 8 electrons:
The valance electron for oxygen is 6, for sulfur is 6, but for hydrogen is 1. Therefore, the molecule has valance electrons. Sulfur is bonded with 4 oxygen atoms, 4 single bonds, whereas 2 hydrogen atoms are bonded with 2 oxygen atoms.

But the actual structure is 2 but it violates octet rule since S is surrounded in this case with 12 electrons

7 0

3 years ago

Read 2 more answers

for the following reaction: 1 CuO + 1 H2 --> 1 Cu +1H2O, what is the quantity of moles of H2O when there are 240 grams of CuO

Ber [7]

Considering the reaction stoichiometry, the quantity of moles of H₂O produced is 3.02 moles.

The balanced reaction is:

CuO + H₂ → Cu + H₂O

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

CuO= 1 mole
H₂= 1 mole
Cu= 1 mole
H₂O= 1 mole

The molar mass of the compounds present in the reaction is:

CuO= 79.55 g/mole
H₂= 2 g/mole
Cu= 63.55 g/mole
H₂O: 18 g/mole

Then, by reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of mass of each compound participate in the reaction:

CuO= 1 mole× 79.55 g/mole= 79.55 grams
H₂= 1 mole× 2 g/mole= 2 grams
Cu= 1 mole× 63.55 g/mole= 63.55 grams
H₂O: 1 mole× 18 g/mole= 18 grams

Then, it is possible to determine the moles of H₂O necessary by the following rule of three: If by reaction stoichiometry 79.55 grams of CuO produces 1 mole of H₂O, 240 grams of CuO produces how many moles of H₂O?

$molesofH_{2} O=\frac{240 grams of CuOx 1 mole ofH_{2} O }{79.55 grams of CuO}$

moles of H₂O= 3.02 moles

Finally, the quantity of moles of H₂O produced is 3.02 moles.

Learn more:

brainly.com/question/11999193
brainly.com/question/15111313?referrer=searchResults
brainly.com/question/9926203?referrer=searchResults
brainly.com/question/6061451?referrer=searchResults

6 0

3 years ago