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riadik2000 [5.3K]
1 year ago
9

Draw lewis formula and structural formula of hydrogen ion please and thank you

Chemistry
1 answer:
tresset_1 [31]1 year ago
4 0

The Lewis formula refers to a diagram showing the distribution of electrones and in case of a molecule it also shows the bonds.

The structural formula on the other hand is a representation of the molecular structure that shows all the atoms that form the molecule, arranged in a three dimentional space,

In this case we have the hydrogen ion, which is the simpliest case we can have.

Hydrogen ion is the hydrogen atom possitively charged as it has lost his electron. Therefore the structural formula is simply the following:

The Lewis formula is also very simple as this ion has no electrons and has no bonding to other atoms:

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What is the OH- of {H+} = 4.0 x 10 to the power of -8
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Answer:

At standard room temperature, [{\rm OH^{-}] \approx 2.5 \times 10^{-7}\; \rm M when [{\rm H^{+}] = 4.0 \times 10^{-8}\; \rm M.

Explanation:

The following equilibrium goes on in water:

{\rm H_{2}O}\, (l) \rightleftharpoons {\rm H^{+}}\, (aq) + {\rm OH^{-}}\, (aq).

The forward reaction is known as the self-ionization of water. The ionization constant of water, K_{\rm w}, gives the equilibrium position of this reaction:

K_{\rm w} = [{\rm H^{+}] \cdot [{\rm OH^{-}}].

At standard room temperature (25\; {\rm ^{\circ}C}), K_{\rm w} \approx 10^{-14}. Also, [{\rm H^{+}}] = 4.0 \times 10^{-8}\; \rm mol \cdot L^{-1}. Substitute both values into the equation and solve for [{\rm OH^{-}}].

\begin{aligned} {[}{\rm OH^{-}}{]} &= \frac{K_{\rm w}}{[{\rm H^{+}}]} \\ &\approx \frac{10^{-14}}{4.0 \times 10^{-8}} = 2.5 \times 10^{-7}\end{aligned}.

In other words, in an aqueous solution at standard room temperature, [{\rm OH^{-}] \approx 2.5 \times 10^{-7}\; \rm M when [{\rm H^{+}] = 4.0 \times 10^{-8}\; \rm M.

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