How To Cacl2: Calcium Chloride

The hypothesis is; as we know the concentration of sodium carbonate (Na2CO3) we can obtain the concentration of hydrochloric acid using the titration of a standard solution.

Cu 2+ (aq) + 2 NO3- (aq) + Na+ (aq) + I- (aq)  CuI (s) + Na+ (aq) + 2 NO3- (aq)

To study the nature of ionic reactions, write balanced equations, and write net ionic equations for precipitation reactions.

Your Finding: Color change occurs and copper is appearing. Reaction 2 Mg + CuSo4→ MgSo4 + Cu Hypothesis: There is going to be a reaction because magnesium is more active than copper. Your Finding: Color change occurs and copper is appearing. Reaction 3 Cu + 2AgNO3 → Cu(No3)2 + 2Ag Hypothesis:

: During each reaction, something happened. During reaction 1, after adding the nitric acid a red-brown gas was created. The copper first turned green after a few minutes turned into a blue solution. Reaction 2, When acid was added a blue precipitate formed. Reaction 3, when heated the solution turned into a black precipitate.

When mixed, none of the metals seemed to react, as none of them emitted gas by bubbling/fizzing and none changed color. This could have been predicted as Magnesium is towards the top of the activity series, and would not have been replaced by Fe, Cu, or Zn as all those are lower on the activity series. The activity series is a guide which helps predicts chemical reactions, as it lists which metals can replace or be replaced by other metals. Part of the reactivity series is as follows, Na>Mg>Zn>Fe>Sn> Pb>H>Cu>Ag.

Write a balanced equation for the synthesis reaction that occurred. The balanced equation for the synthesis reaction that occurred in experiment 1 is: 2Mg + O2 → 2MgO. Experiment 2 1. A hydrate is a chemical compound that has water molecules bound loosely to it by electrostatic forces.

These combinations were as follows: Iron (III) Nitrate and Sodium Phosphate Iron (III) Nitrate and Sodium

Reaction B: Cu(NO3)2(aq)+ 2NaOH(aq) → Cu(OH)2(s)+ 2NaNO3(aq) Reaction C: Cu(OH)2(s) → CuO(s)+ H2O(l) Reaction D: CuO(s)+ H2SO4(aq) → CuSO4(aq)+ H2O(l) Reaction E: CuSO4(aq)+ Zn(s) →ZnSO4(aq)+ Cu(s) ZnSO4(aq)+ H2SO4(aq) →ZnSO4(aq)+

The reason why Na2SO4 only reacts with Ca(NO3)2 is because when sulfate combines with calcium (or Ag, Sr, Ba, Pb), it becomes insoluble. In the other reactions, copper, nickel, and zinc were all soluble when combined with sulfate. Also, no precipitate formed when mixed with KI because both elements in the molecule are soluble when combined with other elements, except for Ag, Pb, and Hg when combined with a halide. This lab shows that some elements and ions are soluble while others are not and that there are some exceptions to the rule. During our first try, my group had few errors.

Express your answer as a balanced chemical equation. Identify all of the phases in your answer.

Then the correct amount of each reactant had to be determined by turning .03 moles into grams and milliliters to use in the experiment.

I believe Calcium + Water -> Calcium Hydroxide + Hydrogen. This is a single replacement reaction type. 1 Ca + 2 H2O -> 1 Ca(OH) + 1 H2 This formula is a single replacement reaction type because only the calcium and the oxygen can switch. Copper(II) Carbonate ->

Reaction two should result in disodium phosphate (Na2HPO4) with a formula weight of 141.96 g/mol and reaction three should achieve monosodium phosphate (NaH2PO4) with a formula weight of 119.98 g/mol.

The reaction between the bicarbonate ion and citric acid produces water, carbon dioxide, and the citrate ion. Write the balanced equation for the reaction.