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KIM [24]
2 years ago
10

Net Ionic Equations for mixing Strong Acids with Strong Bases Consider a reaction between hydrochloric acid and potassium hydrox

ide.
a) In an aqueous solution of hydrochloric acid, check all of the major species found in solution (ignore the trace hydronium ions and hydroxide ions that would come from the autoionization of water). HCI (1) CIo (aq) CI (aq) OH (ag)H20 () H3o (aq)
b) In an aqueous solution of potassium hydroxide, check all of the major species found in solution (ignore the trace hydronium ons and hydroxide ions that would come from the autoionization of water). H20 () K+ (aq) OH (aq) Hyo (aq) KOH (5)
c) When the acid and base react together, they will neutralize each other to form water and a salt. Give the chemical formula for the salt formed. chemPad Help Greek acid and potassium hydroxide. Write it out in this order. Remember that, by convention, a net ionic equation has a single reaction arrow
d) When you cancel out the spectator ions, what is the net ionic equation that remains for the reaction between hydrochloric Help chemPad Oreek ▼
Chemistry
1 answer:
AleksandrR [38]2 years ago
4 0

Answer:

sorry but I am just answering the questions because I need points

Explanation:

thank you

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A _____ ionic compound is a polyatomic ionic compound composed of three or more different elements.
Ghella [55]

Answer:

ternary

Explanation:

7 0
3 years ago
0.5mol/dm3 hydrochloric acid is added gradually to a flask containing 20cm3 of 2 mol/ dm3 sodium hydroxide solution.
sweet-ann [11.9K]

Answer:

The answer is B which is 40

7 0
2 years ago
Consider the reversible reaction, A+B⇌C+D. If the concentration of product D is increased, the rate of the reverse reaction woul
natali 33 [55]

Answer:

If the concentration of product D is increased, the rate of the reverse reaction would increase.

Explanation:

Chemical reaction:

A + B ⇄ C + D

In given condition the equilibrium is disturb by increasing the concentration of product.

When the concentration of product D is increased the system will proceed in backward direction in order to regain the equilibrium. Because when the product concentration is high it means reaction is not on equilibrium state the reaction will proceed backward direction to regain the equilibrium state.

According to the Le- Chatelier principle,

At equilibrium state when stress is applied to the system, the system will behave in such a way to nullify the stress.

The equilibrium can be disturb,

By changing the concentration

By changing the volume

By changing the pressure

By changing the temperature

4 0
3 years ago
Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), K1 = 9.57×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), K2 = 1.46×10−19, what is the equilib
Dvinal [7]

<u>Answer:</u> The value of K_c for the final reaction is 7.16\times 10^{25}

<u>Explanation:</u>

The given chemical equations follows:

<u>Equation 1:</u>  H_2S(aq.)\rightleftharpoons HS^-(aq.)+H^(aq.);K_1

<u>Equation 2:</u>  HS^-(aq.)\rightleftharpoons S^{2-}(aq.)+H^(aq.);K_2

The net equation follows:

S^{2-}(aq.)+2H^+(aq.)\rightleftharpoons H_2S(aq.);K_c

As, the net reaction is the result of the addition of reverse of first equation and the reverse of second equation. So, the equilibrium constant for the net reaction will be the multiplication of inverse of first equilibrium constant and the inverse of second equilibrium constant.

The value of equilibrium constant for net reaction is:

K_c=\frac{1}{K_1}\times \frac{1}{K_2}

We are given:

K_1=9.57\times 10^{-8}

K_2=1.46\times 10^{-19}

Putting values in above equation, we get:

K_c=\frac{1}{(9.57\times 10^{-8})}\times \frac{1}{(1.46\times 10^{-19})}=7.16\times 10^{25}

Hence, the value of K_c for the final reaction is 7.16\times 10^{25}

5 0
3 years ago
How many grams are in 0.5 moles C6H12O6?<br><br><br><br> Show work please!
Nitella [24]
Molar mass of C6H12O6 = 6x12 + 12x1 + 6x16 = 180g

SO mass of 1 mole of C6H12O6 = 180g

mass of 0.5 mole of C6H12O6 = 0.5 x180g = 90g

6 0
3 years ago
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