Problem: What is the pH of a 0.0150 M aqueous solution of rubidium hydroxide (RbOH)?A. 1.82B. 6.20C. 10.8D. 12.2E. none of the above
FREE Expert Solution
We’re being asked to determine the pH of a 0.0150 M aqueous solution of rubidium hydroxide (RbOH).
Let’s first determine what type of base is RbOH:
• Any Group 1A metal when combined with OH-, H-, O2- or NH2- makes a strong base
• Rb (Group 1A metal) is paired with OH-
• RbOH → strong base
We're going to calculate the pH of the solution using the following steps:
Step 1: Determine the OH- concentration in the solution.
Step 2: Calculate for pOH.
Step 3: Calculate for pH.
Problem Details
What is the pH of a 0.0150 M aqueous solution of rubidium hydroxide (RbOH)?
A. 1.82
B. 6.20
C. 10.8
D. 12.2
E. none of the above
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Rabeony's class at RUTGERS.