The concentration of a stock solution of acetic acid is 2.70 M. If you remove 10.00 mL of this solution and dilute it to 500.0 mL, what will be the molarity
of the diluted solution?

What was bohr’s contribution to the planetary model

Convert the temperature of dry ice, –77 ∞c, into degrees fahrenheit and kelvin.

Percent ionization for a weak acid (ha) is determined by the following formula: percent ionization=[ha] ionized[ha] initial×100%for strong acids, ionization is nearly complete (100%) at most concentrations. however, for weak acids, the percent ionization changes significantly with concentration. the more diluted the acid is, the greater percent ionization.a certain weak acid, ha, has a ka value of 9.4×10? 7.part acalculate the percent ionization of ha in a 0.10 m solution.part bcalculate the percent ionization of ha in a 0.010 m solution