What are the classes of acids and bases? Be specific and give examples, and discuss the concept of pH.

II. Answer the following questions: 1) In the year 1618, England was experiencing a drought. Despite the shortage of water, cattle refused to drink from a certain pond in Epson Common. A man named Henry Wicker took some interest in this, and went over and drank a bit of the water himself. It tasted terribly bitter. He took some home and after boiling off the water he was left with Magnesium Sulfate crystals. This salt became known as "Epsom Salts" and soon after they were being used to treat constipation all over Europe. The three naturally occurring isotopes of magnesium are: magnesium-24(23.985 amu), magnesium-25(24.986 amu) and magnesium-26(26.983 amu). Their percent abundances in nature are 78.99%, 10.00% and 11.01% respectively. What is the average atomic mass of magnesium? 2) There are four naturally occurring isotopes of iron: iron-56 (91.754% at 55.935amu), iron-54 (5.845% at atomic mass of iron? 53.940 amu), iron-57 (2.119% at 56.935 amu) and iron-58 (0.2830% at 57.933 amu).…

Le Simple Markup A Previc Show Markup A Next Delete Previous Next Eraser Pen Comments Comment New Show Ink Track Accept Reject Comment Changes Reviewing Pane Comments Tracking Changes 4.Suppose you run a titration of an acid yourself. You do it three times be- tween an acid and sodium hydroxide solution. Here is some data: Average volume of sodium hydroxide solution delivered: 9.10 mL Concentration of sodium hydroxide standard solution: 0.1010 M Average mass of acid solution: 9.555 g The average volume of sodium hydroxide solution is the average of three titra- tions. In other words, you did the experiment three times and took an average. The same goes for the average mass of the acid. You ran the experiment three times and the average mass of the acid solution is given for those three titra- tions. The sodium hydroxide solution was standardized and the concentration is given. Show your step-by-step calculations for this experiment to find the mass per- cent of acid in the solution.…

Will 260 milligrams of calcium carbonate raise the pH of 75.0 milliliters of stomach fluid from a low pH of 1.0 into the normal pH range of 1.5-3.5? The first step of this problem is to convert 260.0mg of calcium carbonate to grams of calcium carbonate. Submit a reply that that tells how you decide approach the problem and shows the work that results in an answer. Use correct units and significant figures. In addition, reply to another student's a