Answer:
0.001 M OH-
Explanation:
[OH-] = 10^-pOH, so
pOH + pH = 14 and 14 - pH = pOH
14 - 11 = 3
[OH⁻] = 10⁻³ ; [OH-] = 0.001 M OH-
Step one write the chemical equation for reaction
= Ag2O + 2(C10H10N4SO2)---> 2 ( AgC10H9N4SO2)
The reacting ratio of Ag2O to AgC10H9N4SO2 is 1:2 from the reaction above
step 2; find the number of moles of AgC10H9N4SO2
that is mass/molar mass
The molar mass of AgC10H9N4SO2 = 107.86 +(12 x10) + (1 x 9) + (4 x 14) +32 +(16 x2) =356.86g/mol
moles is therefore= 25g/356.86g/mol= 0.07moles
by use of mole ratio the moles of Ag2O= 0.0702=0.035moles
mass = moles x molar mass
the molar mass of Ag2O=231.72 g/mol
mass is therefore= 231.72g/mol x 0.035moles= 8.11grams
I guess it is D, bc heterogeneous means a mixture that’s not uniform in structure
<h3>
Answer:</h3>
318.405 g
<h3>
Explanation:</h3>
We are given;
- Volume of K₃PO₄ solution to be prepared as 750.0 mL or 0.75 L
- Molarity of the solution to be prepared as 2.00 M
We are required to determine the mass of K₃PO₄ to be measured.
<h3>Step 1: Determine the number of moles of K₃PO₄</h3>
Molarity = Moles ÷ Volume
Rearranging the formula;
Number of moles = Molarity × Volume
Therefore;
Moles of K₃PO₄ = 2.00 M × 0.75 L
= 1.5 moles
<h3>Step 2: Determine the mass of K₃PO₄ to be measured</h3>
Mass = Number of moles × Molar mass
Molar mass of K₃PO₄ = 212.27 g/mol
Therefore;
Mass of K₃PO₄ = 1.5 moles × 212.27 g/mol
= 318.405 g
Therefore, the mass of K₃PO₄ that should be weighed is 318.405 g
Answer:
Please take this hepful hint :
F = m * a
6.2 = 2.3 * a
a = 2.7 m/s^2
Explanation:
