I am really stuck on these 2 questions:
1. Why was 2M HNO3 added before adding 0.05M AgN03?
2.Write a full equation b.) an ionic equation between silver nitrate solution and sodium chloride solution.
In the future, PLEASE tell us what you are doing. I am guessing that you have added AgNO3 to a Cl solution to ppt AgCl. The reason you add HNO3 is because you want an acid solution from which to ppt AgCl. AgOH and/or Ag2O (actually a hydrated silver oxide) ppts from a neutral or basic solution.
AgNO3(aq) + NaCl(aq) ==> AgCl(s) + NaNO3(aq)
Ag^+ + NO3^- + Na^+ + Cl^- ==> AgCl(s) + Na^+ + NO3^-
Net ionic:
Ag^+(aq) + Cl^-(aq) ==> AgCl(s)
B (AQ) + AGNO3 (AQ) OBSERVATION GIVES A WHITE PERCIPTATE WHAT IS THEINFERENCE
To answer your first question, "Why was 2M HNO3 added before adding 0.05M AgNO3?", it seems that you are referring to a specific chemical reaction. Without additional context, it is difficult to give a definitive answer. However, I can provide you with some general information that might help.
Adding a strong acid, such as 2M HNO3, before adding 0.05M AgNO3 could serve a few different purposes, depending on the specific reaction being conducted. Here are a couple of possible reasons:
1. Acidification: The addition of HNO3 may be used to acidify the reaction environment. Acidification can help in preventing the precipitation of certain compounds and improve the solubility or reactivity of other components.
2. Neutralization: In some cases, if the reaction involves the formation of a precipitate, the addition of HNO3 may be used to neutralize any basic (alkaline) species in the solution. By neutralizing the basic components, the reaction conditions can be controlled, allowing for more controlled precipitation or reaction.
It's important to note that without further details about the specific experiment or context, these are just general possibilities. The reasons for adding 2M HNO3 could vary depending on the experimental objectives or the desired reaction conditions.
Moving on to your second question, writing the full ionic equation between silver nitrate (AgNO3) solution and sodium chloride (NaCl) solution can be done as follows:
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
This equation represents a precipitation reaction, where silver chloride (AgCl) is formed as a solid precipitate, while sodium nitrate (NaNO3) remains in the aqueous state.
However, if you specifically request the ionic equation, we need to represent the dissociation of the soluble ionic compounds into their respective ions:
Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) → AgCl(s) + Na+(aq) + NO3-(aq)
In the above equation, the ions that are involved in the reaction are shown, while the spectator ions (Na+ and NO3-) are not included in the final equation since they do not participate in the actual reaction.
I hope this helps clarify your questions! If you have any further inquiries or need more specific information, feel free to ask.