An element has two naturally-occurring isotopes. The mass numbers of these isotopes are 123 amu and 125 amu, with natural abundances of 95% and 5%, respectively. Calculate its average atomic mass. Report your answer to 1 decimal place.

123.1

Explanation:

The average atomic mass of an element which exhibits isotopy is the average mass of its various isotopes as they occur naturally in any quantity of the element.

Average atomic mass = (95% of 123 amu)+(5% 0f 125 amu)

= (0.95 × 123) + (0.05 × 125)

= 116.85 + 6.25

= 123.1   (to 1 decimal place)

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.