Concentration of H+ ions in HNO3 solution is 10⁻¹ which is equal to 0.1 M
![\bf \: pH \: = - log[{h}^{ + }]](https://tex.z-dn.net/?f=%20%5Cbf%20%20%5C%3A%20pH%20%5C%3A%20%20%3D%20%20-%20log%5B%7Bh%7D%5E%7B%20%2B%20%7D%5D)
putting the value we get
![\sf \dashrightarrow \: pH \: = - log \: [ \frac{1}{10}] \\ \\ \sf \dashrightarrow \: pH \: = - log \: {10}^{ - 1} \\ \\ \sf \dashrightarrow \: pH \: = 1](https://tex.z-dn.net/?f=%20%20%5Csf%20%5Cdashrightarrow%20%20%5C%3A%20pH%20%5C%3A%20%20%3D%20%20-%20log%20%5C%3A%20%5B%20%5Cfrac%7B1%7D%7B10%7D%5D%20%5C%5C%20%20%5C%5C%20%5Csf%20%5Cdashrightarrow%20%20%5C%3A%20pH%20%5C%3A%20%3D%20%20%20-%20log%20%5C%3A%20%7B10%7D%5E%7B%20-%201%7D%20%20%5C%5C%20%20%5C%5C%20%5Csf%20%5Cdashrightarrow%20%20%5C%3A%20pH%20%5C%3A%20%3D%201)
So, the required option is A) 1
Consider the equation for calculating molarity: (no. of mole of solute)÷(volume of solution)
First, let's find the no. of mole of solute in AgNO3. As (no. of mole) = mass / molar mass
no. of mole of 85.0g of AgNO3 = 85.0/(107.9+14.0+16.0x3)
=0.5mol
Since the volume of the solution has to be in dm3, just divide the volume in cm3 by 1000 to get the volume in dm3.
Volume of solution = 500/1000
= 0.5 dm3
Therefore, the molarity is
0.5/0.5
=1.0M
The answer should be B.
Answer:
The outermost energy shell of an atom likes to be full with 8 electons
Explanation:
Answer:
B) The molecules were closer together when the juice pop was frozen.
The Keq for the reaction N₂ + 3H2 = 2NH3 if the equilibrium concentrations are Keq = 1.5. The correct option is D.
<h3>What is Keq?</h3>
Keq is the ratio of the concentration of reactant to the concentration of the product.
The balanced equation is
N₂ + 3H₂ = 2NH₃
The equilibrium constant is ![\rm \dfrac{[NH_3]^2}{[N_2]\; [H_2]^3}](https://tex.z-dn.net/?f=%5Crm%20%5Cdfrac%7B%5BNH_3%5D%5E2%7D%7B%5BN_2%5D%5C%3B%20%5BH_2%5D%5E3%7D)
The given concentrations of the compounds have been:
Ammonia = 3 M
Nitrogen = 1 M
Hydrogen = 2 M

Thus, the correct option is D. Keq = 1.5.
Learn more about Keq
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