In order to deprotonate an acid, we must remove protons in order to achieve a more stable conjugate base. For this example, we can use the relationship between carboxylic acid and hydroxide.
Deprotonation is the removal of a proton from a specific type of acid in reaction to its coming into contact with a strong base. The compound formed from this reaction is known as the conjugate base of that acid. The opposite process is also possible and is when a proton is added to a special kind of base. This is a process referred to as protonation, which forms the conjugate acid of that base.
For the example we have chosen to give, the conjugate base is the carboxylate salt. This would be the compound formed by the deprotonated carboxylic acid. The base in question was strong enough to deprotonate the acid due to the greater stability offered as a conjugated base.
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<span>The following is the role of NaCl and EDTA in DNA isolation, hope it helps:
NaCl provides Na+ ions that will block negative charge from phosphates on DNA.
Negatively charged phosphates on DNA cause molecules to repel each other. The Na+ ions will form an ionic bond with the negatively charged phosphates on the DNA, neutralizing the negative charges and allowing the DNA molecules to come together.</span>
Answer:
If the nitrogen atom is a neutral atom, it will have seven electrons orbiting the nucleus of the atom. This is because neutral atoms get their neutral...
Explanation:
Answer:
Moles of boron trifluoride gas that were collected = 11.6 mol
Mass of boron trifluoride gas that were collected = 787 g
Explanation:
Given that:
Temperature = 2.0 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (2.0 + 273.15) K = 275.15 K
V = 15.0 L
Pressure = 0.130 atm
Using ideal gas equation as:
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L atm/ K mol
Applying the equation as:
0.130 atm × 15.0 L = n ×0.0821 L atm/ K mol × 275.15 K
⇒n = 11.6 mol
<u>Thus, Moles of boron trifluoride gas that were collected = 11.6 mol
</u>
Molar mass of boron trifluoride gas = 67.82 g/mol
The formula for the calculation of moles is shown below:
Thus,
<u>Mass of boron trifluoride gas that were collected = 787 g</u>
