A weak acid, HA, has a Ka value of 7.6 * 10-7. Calculate the percent dissociation of HA in a 0.10 M solution and in a 0.010 M solution. Express your answer as a percent using two significant figures. Note that percent dissociation is determined by the formula % dissociation = (HA) dissociated / (HA) initial *100%, and that percent dissociation increases with increasing Ka. Strong acids dissociate completely (100%), while weak acids have a percent dissociation that changes with concentration - the more diluted the acid is, the greater the percent dissociation.