Zn (s) + Cu(NO3)2 (aq) → Cu(s) + Zn(NO3)2 (aq) (Eq. 2) Regarding, the copper and sodium chloride, no visible change occurred after 5 minutes had passed. The copper metal remained at the bottom of the test tube undeterred by the NaCl. There may not have been a reaction because copper is lower on the reactivity series than sodium. Metathesis: Precipitation (Nonredox) The reaction between and KCl is a double replacement reaction because the cations Cu2+ and K+ switched places and formed two new compounds, copper (II) chloride and potassium nitrate. However, there was no observed precipitation in the resulting solution as both are soluble. Balanced formula- Cu(NO3)2(aq) + 2KCl(aq) → CuCl2(aq) + 2KNO3(aq) (Eq. 3) Total ionic- Cu2+(aq) + 2NO3-(aq) …show more content…
As 10 mL of NaOH was added drop wise, the solution began to have a pink tint. The fuchsia color did not permanently stay until 9mL of NaOH was added. The pH indicator demonstrated when exactly the reaction has neutralized. Because an acid and a base reacted to form water and a salt, the reaction is a neutralization …show more content…
9) Total ionic- Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) → Na+(aq) + Cl-(aq) + H2O(l) (Eq. 10) Net ionic- NaOH(s) + H+ (aq) → H2O(l) + Na+ (aq) (Eq. 11) Solid sodium hydrogen carbonate and HCl reacted violently, bubbling and foaming at a rapid pace. NaHCO3, baking soda in layman’s terms, is basic so it reacts strongly with acids such as HCL. Balanced formula- NaHCO3(s) + HCl(aq) → NaCl(aq) + CO2(g) + H2O(l) (Eq. 12) Total ionic- H+(aq) + Cl-(aq) + Na+(aq) + HCO3-(aq) → Na+(aq) + Cl-(aq) + CO2(g) + H2O(l) (Eq. 13) Net ionic- HCO3-(aq) + H+(aq) → H2O(l) + CO2(g) (Eq. 14) Metathesis- Amphoteric Hydroxides and Complex Ion Formation A diluted NaOH solution was created by mixing 6 drops of 4.0 M NaOH and 44 drops of distilled water. 20 drops is equivalent to 1 mL of liquid[E] so the new molarity of the solution can be calculated using an equation used for dilution calculations: M1V1 = M2V2[F] (Eq. 15) (4.0 mol/L)(0.3 mL) = (M2)(2.5 mL) M2 = 0.48 M
CL-, as the ions of H+ and OH- react to form H2O. These spectator ions
We were then to make a base solution of 0.7 M NaOH. In order to standardize
Ionic Equation: H+(aq) + NO3(aq) + Na+(aq) + OH-(aq) → Na+(aq) + NO3(aq) + H2O(l)
The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so
It is important however to note that the NH4 and K ions are still in
Na2S203 (aq) + 2HCl (aq) -> 2NaCl (aq) + H20 (l) + SO2 (g) + S (s)
Neutralization Experiment AIM:- To investigate how heat is given out in neutralizing sodium hydroxide (NaOH) using different concentrations of Hydrochloric Acid. Background Information:- Substances that neutralize acids are called alkalis. An acid is a substance that forms hydrogen ions (H+ ) when placed in water. It can also be described as a proton donor as it provides H+ ions. An example of an acid is hydrochloric acid (HCl), Sulphuric acid (H2SO4) etc.
Compared to the 0.5 M hydrochloric acid that was less concentrated, the more concentrated 2 M hydrochloric acid c...
Rate of Reaction Between Calcium Carbonate and Hydrochloric Acid Plan: In my experiment I will measure the rate of reaction between calcium carbonate and hydrochloric acid. The rate of the reaction is the speed that the reaction takes place so by measuring the rate I will measure the amount of time the reaction takes. Hydrochloric acid is a strong acid that is found in digestive juices in the stomach, it is also used for cleaning metals before they are coated. Calcium carbonate has a few forms including chalk and limestone the main use of these two materials is in the making of concrete, which is used for many things such as buildings. When you put calcium carbonate and hydrochloric acid together they react to form calcium chloride, carbon dioxide and water.
From the unit of chemistry in grade ten science, the students have learned many things from different types of elements in the chart all the way to how each element impacts the daily life each student or even adult lives in. Some of the things I as a student have learned include how to draw the different elements in a bohr rutherford diagram, balancing chemical equations, types of chemical reactions, and even information about the different types of acids and bases. Although there were many other things in the unit, these four definately helped me learn about chemistry in a more in-depth way, as well as teaching me something very new since these were some things a few of the students had never done in the previous years. Learning this in the classroom has really opened my eyes to the world in which we live in today, many times I leave the house on a cold day and as I look upon the cold water becoming ice or even the snow falling down, I know how it is happening, why it is happening, and I can even picture the molecules solidifying as we had seen in class with many different diagrams.
The simplest experiment for this type of situation would be to use red and blue litmus paper to distinguish between acids, bases and salts. Hydrochloric acid (HCl) makes blue litmus paper change color going from blue to red, making it an acid. Sodium hydroxide (NaOH) makes red litmus paper change color going from red to blue, making it a base. Sodium chloride solution (NaCl) is neutral, since it would only soak blue and red litmus paper, considering that it is a by product of when an acid and a base mix together, neutralizing each other.
borate) and 1.0 g. of sodium hydroxide in 20 mL of warm water. It may
For this experiment we used titration to standardize the exact concentration of NaOH. Titration is the process of carefully adding one solution from a buret to another substance in a flask until all of the substance in the flask has reacted. Standardizing is the process of determining a solutions concentration. When a solution has been standardized it is referred to as a standard solution. To know when a solution is at its end point an indicator is added to acidic solution. An indicator is an organic dye that is added to an acidic solution. The indicator is one color is in the acidic solution and another color in the basic solutions. An end point occurs when the organic dye changes colors to indicate that the reaction is over (Lab Guide pg. 141).