What happens to traits when mutations happen

An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric f

aivan3 [116]

Answer:

a. 3.8856x10⁻³M HCl

b. 1.23x10⁻⁴M OH⁻

c. 1.23x10⁻⁴M Ag⁺

d. Ksp = [Ag⁺] [OH⁻]

Explanation:

a. The reaction that you are studying is:

HCl(aq) + AgOH(aq) → H₂O(l) + AgCl(s)

The HCl solution is diluted from 10.00mL to 250.00mL, that is:

250.00mL / 10.00mL = <em>25 -The solution is diluted 25 times-</em>

As original concentration of HCl is 0.09714M, the concentration of the diluted solution is:

0.09714M / 25 =

b. 1 mole of HCl reacts per mole of AgOH, moles of HCl that reacts are:

7.93mL = 7.93x10⁻³L × (3.8856x10⁻³mol HCl / L) = 3.0813x10⁻⁵ moles of HCl.

Based on the reaction, you have in solution

<em>3.0813x10⁻⁵ moles of AgOH = Ag⁺ = OH⁻</em>

The AgOH solution was 250.0mL = 0.2500L, its concentration is:

3.0813x10⁻⁵ moles OH⁻ / 0.2500L =

c. In solution, AgOH produce Ag⁺ and OH⁻ in equals proportions, that means:

1.23x10⁻⁴M OH⁻ =

d. The solubility product reaction of AgOH(s) is:

AgOH(s) ⇄ Ag⁺(aq) + OH⁻(aq)

Where Ksp for this reaction is defined as:

5 0

3 years ago

For the reaction PCl5(g) <--> PCl3(g) Cl2(g) at equilibrium, which statement correctly describes the effects of increasing

xenn [34]

The given question is incomplete. The complete question is :

For the reaction $PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)$ at equilibrium, which statement correctly describes the effects of increasing pressure and adding $PCl_5$ , respectively

a) Increasing pressure causes shift to reactants, adding $PCl_5$ causes shift to products.

b) Increasing pressure causes shift to products ,adding $PCl_5$ causes shift to reactants.

c) Increasing pressure causes shift to products, adding $PCl_5$ causes shift to products.

d) Increasing pressure causes shift to reactants,adding $PCl_5$ causes shift to reactants

Answer: Increasing pressure causes shift to reactants, adding $PCl_5$ causes shift to products.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

$PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)$

a) If the pressure is increased, the volume will decrease according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. As the number of moles of gas molecules is lesser at the reactant side. So, the equilibrium will shift in the left direction. i.e. towards reactants.

b) If $PCl_5$ is added, the equilibrium will shift in the direction where $PCl_5$ is decreasing. So, the equilibrium will shift in the right direction. i.e. towards products.

8 0

2 years ago

in a chemical reaction known as decomposition, carbonic acid breaks down into water, and what other compound?

BartSMP [9]

Answer: it’s carbon dioxide

Explanation:

This is it because decomposition takes place when carbonic acid breaks down So that’s why I put carbon dioxide

8 0

2 years ago

Read 2 more answers

A substance has 55.80% carbon, 7.04% Hydrogen, and 37.16% Oxygen. What is it's empirical and molecular formula if it has a mola

hjlf

55.80 C/12= 4.65/2.3225= 2

7.04 H/1= 7.04/2.3225= 3

37.16 O/16= 2.3225/2.3225= 1

Empirical Formula= C2H3O

301.35/43= 7

(C2H3O)7= C14H21O7= Molecular Formula

5 0

3 years ago

Read 2 more answers

Suppose the reaction system below has already reached equilibrium. Predict the effect that each of the following changes will ha

WARRIOR [948]

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

On removal of reactant from equilibrium reaction ,shifts the equilibrium in backward direction.
On addition of reactant from equilibrium reaction ,shifts the equilibrium in forward direction.
On removal of product from equilibrium reaction, shifts the equilibrium in forward direction.
On addition of product from equilibrium reaction, shifts the equilibrium in backward direction.

$UO_2(s) + 4 HF(g)\rightleftharpoons UF_4(g) + 2 H_2O(g)$

1. Water vapor is removed

On removal of water vapor from equilibrium will decrease the product which will lead to moving forward of an equilibrium that is equilibrium will shift to right direction.

2. $UF_4(g)$ is added

On addition of $UF_4(g)$ from equilibrium will increase the reactant which will lead to moving forward of an equilibrium that is equilibrium will shift to right direction.

3.The reaction is done in a glass reaction vessel. HF(g) attacks and reacts with the glass

Due to reaction of HF with glass will result in decrease in amount of HF present at equilibrium. So, order to counter this equilibrium will shift in backward direction or in left direction.

4. If the reaction is endothermic, and you want to make the equilibrium shift to the right to maximize the products, would you heat or cool the reaction vessel.

I endothermic reaction , heat is added to the reaction for which we can treat heat as a reactant.Now, we want to shift the equilibrium to right which means in the forward direction.

And this can be done by increasing the reactant amount, here by adding more heat to the equilibrium will shift the reaction to the right side.

So, for increasing heat we will heat the reaction vessel.

5 0

2 years ago