Suppose you titrate 80.0 ml of 2.00 m naoh with 20.0 ml of 4.00 m hcl. what is the final concentration of oh− ions.

In a sample of oxygen gas at room temperature, the average kinetic energy of all the balls stays constant. which postulate of kinetic molecular theory best explains how this is possible? a. attractive forces between gas particles are negligible because the particles of an ideal gas are moving so quickly. b. collisions between gas particles are elastic; there is no net gain or loss of kinetic energy. c. gases consist of a large number of small particles, with a lot of space between the particles. d. gas particles are in constant, random motion, and higher kinetic energy means faster movement.

Suppose you wanted to make 100 grams of water. what is the molar mass of water (h2o)?

Which element is least likely to undergo a chemical reaction