1. In step 3, hydroxide ions reacted with and removed H+ ions from solution (see Equation 3). What color change was observed when NaOH was added? Which substance (HIn or In) increased in concentration as a result? 1. Explain the observed color change: Removing one of the products from an equilibrium mixture of reactants and products decreases the rate of the (forward/reverse) reaction and thus (increases/decreases) the amount of product. What form(s) of the indicator were most likely present when the transition color was observed in step 5? How does this observation provide visual evidence that not all reactions "go to completion?"

Lowest 1A Highest 8A H2A Li Be Na Mg 38 48 58 68 7888 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Ha 3A 4A 5A 6A 7A He B C N O F Ne 18 2B Al Si P S Cl Ar Using only the periodic table arrange the following elements in order of increasing ionization energy: neon, helium, argon, radon. Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Cf Es Fm Md No Lr

In a titration experiment, 29.1 mL of 0.953 M HCOOH neutralizes 23.2 mL of Ba(OH)₂. What is the concentration of the Ba(OH), solution? Round your answer to 3 significant digits. M 0x10 X 5

A chemistry student weighs out 0.112 g of formic acid (HCHO2) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0800M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Be sure your answer has the correct number of significant digits.