Answer:
7.60 M
Explanation:
Our method to solve this question is to use the definition of molarity (M) concentration which is the number of moles per liter of solution, so for this problem we have
[Cl⁻] = # mol Cl⁻ / Vol
Now the number of moles of Cl⁻ will be sum of Cl in the 1.00 mL 5.4 M solution plus the moles of Cl⁻ in the 0.50 mL 12 M H . Since the volume in liters times the molarity gives us the number of moles we will have previous conversion of volume to liters for units consistency:
1mL x 1 L / 1000 mL = 0.001 L
0.5 mL x 1L/1000 mL = 0.0005 L
[Cl⁻] = 0.001 L x 5.4 mol/L + 0.0005L x 12 mol/L / ( 0.001 L + 00005 L )
= 7.6 M
This is the same as the statement given in the question.
Answer: The concentration of hydroxide ions at this temperature is 
Explanation:
When an expression is formed by taking the product of concentration of ions raised to the power of their stoichiometric coefficients in the solution of a salt is known as ionic product.
The ionic product for water is written as:
![K_w=[H^+][OH^-]](https://tex.z-dn.net/?f=K_w%3D%5BH%5E%2B%5D%5BOH%5E-%5D)
![5.13\times 10^{-13}=[H^+][OH^-]](https://tex.z-dn.net/?f=5.13%5Ctimes%2010%5E%7B-13%7D%3D%5BH%5E%2B%5D%5BOH%5E-%5D)
As ![[H^+]=[OH^-]](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%3D%5BOH%5E-%5D)


The concentration of hydroxide ions at this temperature is 
Answer:
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