Use your knowledge about solubility rules and reactions to write (1) a balanced chemical  equation (molecular equation), (2) a total ionic equation, and (3) a net ionic equation for the  reactions below. Include the appropriate phase for each species. Do your experimental  observations match your predictions? (m) Na2CO3(aq) + SrCl2(aq) →

You are performing an experiment in lab that involves the titration of 25.0 mL of H2SO4 solution. You titrate the acidic solution with 0.5751 M NaOH and the equivalence point is reached by the addition of 18.49 mL of NaOH solution. Using the balanced equation below, calculate the Molarity of H2SO4 in the flask. Do NOT include units or write the answer in scientific notation. 2NaOH(aq) + H2SO4(aq) → 2H2O(l) + Na2SO4(aq)

A chemistry student weighs out 0.159 g of ascorbic acid (H,C,H,0), a diprotic acid, 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 final equivalence point. Be sure your answer has the correct number of significant digits. mL

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type solution initial components (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral A B 09 C D H₂O H₂O H₂O, HCIO H₂O, HCIO4 0000000 change add HI add KI add NaClO add NaOH effect of change on pH (check one) O pH higher O pH lower OpH the same O pH higher O pH lower OpH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same