35
Because there’s 7 carbon atoms in every molecule of artificial sweetener
And if you have 5 molecules of that
7x5 =35
Answer:
(3) NaNO₃
Step-by-step explanation:
Sodium nitrate has ionic bonds, because it consists of Na⁺ and NO₃⁻ ions.
However, the nitrate ions have <em>covalent bonds</em> between the O atoms and the central N atoms.
(1) and (2) are <em>wrong</em>. Both N₂O₅ and HCl consist of nonmetals, so they are <em>covalent</em> compounds.
(4) is <em>wrong</em>. NaCl has <em>only ionic bonds</em> between the Na⁺ and Cl⁻ ions
The percent composition<span> gives you only the empirical formula.
</span><span>To get the molecular formula, you must either know the molecular mass or do an experiment to find it.</span>
Answer:
A) pH of Buffer solution = 4.59
B) pH after 5.0 ml of 2.0 M NaOH have been added to 400 ml of the original buffer solution = 4.65
Explanation:
This is the Henderson-Hasselbalch Equation:
![pH = pKa + log\frac{[conjugate base]}{[acid]}](https://tex.z-dn.net/?f=pH%20%3D%20pKa%20%2B%20log%5Cfrac%7B%5Bconjugate%20base%5D%7D%7B%5Bacid%5D%7D)
to calculate the pH of the following Buffer solutions.
Answer:
Approximately
.
Explanation:
Balanced equation for this reaction:
.
Look up the relative atomic mass of elements in the limiting reactant,
, as well as those in the product of interest,
:
Calculate the formula mass for both the limiting reactant and the product of interest:
.
.
Calculate the quantity of the limiting reactant (
) available to this reaction:
.
Refer to the balanced equation for this reaction. The coefficients of the limiting reactant (
) and the product (
) are both
. Thus:
.
In other words, for every
of
formula units that are consumed,
of
formula units would (in theory) be produced. Thus, calculate the theoretical yield of
in this experiment:
.
Calculate the theoretical yield of this experiment in terms of the mass of
expected to be produced:
.
Given that the actual yield in this question (in terms of the mass of
) is
, calculate the percentage yield of this experiment:
.