Determine whether the following hydroxide ion concentrations ([OH−]) correspond to acidic, basic, or neutral solutions by estimating their corresponding hydronium ion concentrations ([H3O+] using the ion product constant of water (Kw). Hydronium ion concentration [H3O+] Solution condition Greater than 1×10−7 M Acidic Equal to 1×10−7 M Neutral Less than 1×10−7 M Basic It may help to keep the following equation in mind as you work Kw = [H3O+][OH−] = [1×10−7 M][1×10−7 M] = 1×10−14 M Drag the appropriate items to their respective bins.

See explanation below

Explanation:

The question is incomplete. However, I managed to find a similar question with these values of [OH⁻]. If these values are not the same that you have, don't worry, you all need to replace your given data in this procedure, and you should get the accurate results. The concentrations here will be:

[OH-]=10x10^-12M

[OH-]=7x10^-9M

[OH-]=7x10^-4M

[OH-]=8X10^-10M

[OH-]=1X10^-5M

[OH-]=4X10^-13M

[OH-]=1X10^-7M

[OH-]=2X10^-2

Now, to get the [H₃O⁺] we just use the following expression:

Kw = [OH⁻] [H₃O⁺] > [H₃O⁺] = Kw / [OH⁻]

Applying this expression, we'll get the hydronium concentrations and then, we could see which one is acidic, basic or neutral:

a) [OH-] = 1x10⁻¹² M

[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻¹² = 0.01 M or 1x10⁻² M. Acidic

b) [OH-]= 7x10⁻⁹ M

[H₃O⁺] = 1x10⁻¹⁴ / 7x10⁻⁹ = 1.43x10⁻⁶ M. Acidic

c) [OH-] = 7x10⁻⁴ M

[H₃O⁺] = 1x10⁻¹⁴ / 7x10⁻⁴ = 1.43x10⁻¹¹ M. Basic

d) [OH-] = 8x10⁻¹⁰M

[H₃O⁺] = 1x10⁻¹⁴ / 8x10⁻¹⁰ = 1.25x10⁻⁵ M. Acidic

e) [OH-] = 1x10⁻⁵M

[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻⁵ = 1x10⁻⁹ M. Basic.

f) [OH-] = 4x10⁻¹³ M

[H₃O⁺] = 1x10⁻¹⁴ / 4x10⁻¹³ = 2.5x10⁻² M. Acidic

g) [OH-] = 1x10⁻⁷ M

[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻⁷ = 1x10⁻⁷ M. Neutral

h) [OH-] = 2x10⁻² M

[H₃O⁺] = 1x10⁻¹⁴ / 2x10⁻² = 5x10⁻¹³ M. Basic.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

yes it is balanced