Author: Anonymous

A KCC student titrated 100.00 mL of a NaOH solution using 55.00 mL of a 0.1000 M H2SO4 solution. How many moles of acid were used ? This is part 1 of a titration problem H2SO4 + 2 NaOH → Na2SO4 + 2 H2O

A 1:20 dilution is done with a 50.0 ppt solution. What is the concentration of the diluted solution ?

What will be the [H3O+1] if 0.001500 moles of HCl is added to 1.000 L of water ? The reaction gives the conversion factor               HCl       +      H2O      →       H3O+1      +       Cl-1  start: 0.001500                                    0                       0 equil:      0                                   –––––––          –––––––note: this is related to the next problem

True or false about the diagram where a cell is placed into the 0.4 osM solution: the cell will swell and lyse due to osmotic pressure

Complete the reaction when ammonia is dissolved into waterNH3   +   H2O    →   __1__   +   __2__      (add letters alphabetically for 1 & 2)the acid is __3__the base is __4__the conjugate acid is __5__the conjugate base is __6__A.  H2O            B.  H3O+1            C.  OH-1             D.  NH4+1              E.  NH3  _______ _______ _______ _______ _______ _______

Pb, element 82, has 78 core electrons and 4 valence electrons

Give the systematic name for Ni(H2PO3)3   (Credit will not be given for older style names)

Please attach your one page SYW here.  Make sure it is legible and in the correct orientation.

Calculate the Ka for lactic acid, HC3H5O3, if in a 1.0000 M solution there is 0.9884 M HC3H5O3 left at equilibrium.                       HC3H5O3      +     H2O      ⇔       H3O+1       +      C3H5O3-1 start:              1.0000 M             55.5 M                  0                           0 equilibrium:   0.9884 M             55.5 M            0.0116 M            0.0116 M

Give the formula for scandium nitrate. Click/Scroll on the U button to get superscripts and subscripts.