Using the Henderson-Hasselbalch equation on the solution before HCl addition: pH = pKa + log([A-]/[HA]) 8.0 = 7.4 + log([A-]/[HA]); [A-]/[HA] = 4.0. (equation 1) Also, 0.1 L * 1.0 mol/L = 0.1 moles total of the compound. Therefore, [A-] + [HA] = 0.1 (equation 2) Solving the simultaneous equations 1 and 2 gives: A- = 0.08 moles AH = 0.02 moles Adding strong acid reduces A- and increases AH by the same amount. 0.03 L * 1 mol/L = 0.03 moles HCl will be added, soA- = 0.08 - 0.03 = 0.05 moles AH = 0.02 + 0.03 = 0.05 moles Therefore, after HCl addition, [A-]/[HA] = 0.05 / 0.05 = 1.0 Resubstituting into the Henderson-Hasselbalch equation: pH = 7.4 + log(1.0) = 7.4, the final pH.
Answer:
Isotopes are atoms of the same element with the same number of protons but different number of neutrons.
Hope this helps.
Is it kinetic or potential energy Or frequency and wavelength
Electric force is given by:
F = (kQ₁Q₂)/r²
where k is Coloumb's constant of value 9 x 10⁹, Q₁ and Q₂ are charges and r is the separation between them.
Let the charge of the nucleus be located at its center.
The separation of the proton is equal to:
Radius of nucleus + distance from surface
= 3 + 1.8
= 4.8 fm
Charge of Nucleus = 54e
Charge of proton = e
F = (9 x 10⁹ x 54 x 1.60 x 10⁻¹⁹ x 1.60 x 10⁻¹⁹)/(4.8 x 10⁻¹⁵)²
F = 540 N
Part 3)
The mass of the proton = 1.67 x 10⁻²⁹ kg
acceleration = 540/1.67 x 10⁻²⁹
= 3.20 x 10³¹ m/s²
Answer:
Explanation:
Explanation:
As you know, the empirical formula tells you what the smallest whole number ratio that exists between the atoms that make up a compound is.
In your case, you know that the empirical formula is
NH Cl
2
, which means that the regardles of how many atoms of each element you get in the actual compound, the ratio that exists between them will always be
1:2:1.
What you actually need to determine is how many empirical formulas are needed to get to the molecular formula.
Notice that the problem provides you with the molar mass of the compound. This means that you can use the molar mass of the empirical formula to determine exactly how many atoms you need to form the compound's molecule.
molar mass empirical formula×n=molar mass compound
To get the molar mass of the empirical formula, use the molar masses of its constituent atoms
14.0067 g/mol+2×1.00794 g/mol+35.453 g/mol=51.48 g/mol≈
51.5 g/mol
This means that you have
51.5g/mol×n=51.5g/mol
As you can see, you have
n=1.
This means that the empirical formula and the molecular formula are equivalent,
NH Cl.
2
