The answer is (2) 2. First of all, a greater hydronium ion concentration means more acidic, so we need a lower pH. Also, you need to remember that pH is on a base 10 log scale. This means that a difference by a factor of 10 in concentration is a difference of 1 on the pH scale. So since the difference is a factor of 100 (10^2), the difference is 2. We already established that the pH must be lower, so your answer is 4 - 2 = 2.
Answer:
c Acid + base = conjugate base + conjugate acid
Explanation:
In a Bronsted-Lowry acid-base reaction, the original acid gives up its proton and becomes a conjugate base. In like manner, the original base accepts a proton and becomes a conjugate acid. For every acid, there is a conjugate base and for every base, there is a conjugate acid:
HA ⇄ H⁺ + A⁻
acid conjugate base
B + H⁺ ⇄ HB⁺
base conjugate acid
This is FALSE.
In the Bible, God created the heavens and the earth.
God said "Let there be light!" and there was.
Answer: False
Happy studying ^-^
One molecule of water contains two atoms of hydrogen and one atom of oxygen, the atomicity of water is three.
if O is -2 and hydrogen +1 then phosphorus is +5
What this tells you is that the oxidation number of P in phosphorus acid must be +3 or +4, while the value for phosphoric acid must be +5 or +6. Since phosphorus is a member of group 5A, it has 5 electrons in its valence shell. As a result, the most common oxidation states it can have are +3 (s2p0) or +5 (s0p0).
So far we have determined the oxidation state at P. What needs to be done now is to add as many oxygens and hydroxyl (OH) to make the molecule neutral. The correct combination will have the correct Lewis-dot structure. For phosphorous acid we need a combination that will add up to +3. This can be done by adding 3 OH- to the central atom to yield the structure H3PO3. There is a little caveat though. Because this is not a hydro___acid, it is implied that there must be at least one oxo ligand (O^2-) bonded to P. Therefore, the actual bonding structure is not P(OH)3 but rather H-P(=O)(OH)2, where one H is bonded directly to the phosphorus atom and is the least acidic of the protons. The great thing is that the oxidation charge of P is still +3 because P is slightly more electronegative than H (some theories will say otherwise); thus the hydrogen is regarded as H+ for this example.
With phosphoric acid, charge of +5, you can have 3 OH- and 1 O^2- to make a neutral molecule:
O=P(OH)3.
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