WORDS: Obiective: To predict the products of some displacement reactions and write net ionic equations. Note-the (aq) has been eliminated from all equations below while (s), (I) and (g) have been used to represent phases. When you write chemical reactions in your lab reports you must show all phases including (aq).

WORDS: Obiective: To predict the products of some displacement reactions and write net ionic equations. Note-the (aq) has been eliminated from all equations below while (s), (I) and (g) have been used to represent phases. When you write chemical reactions in your lab reports you must show all phases including (aq).

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 35QRT

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Write the objectives IN YOUR OWN WORDS: To predict the products of some displacement reactions and write net ionic equations. Note-the (aq) has been eliminated from all equations below while (s), (1) and (g) have been used to represent phases. When you write chemical reactions in your lab reports you must show all phases including (aq).
For 14 reactions from this experiment in which there is a driving force, give the balanced molecular, ionic and net ionic equations. Then identify the driving force for each reaction. Be sure to include the proper state symbols (e.g., aq, s, I, or g) for all substances. For each type of driving force, be sure to include at least one example (e.g., precipitation, gas formation, neutralization).
You are required to standardize a dilute solution of sulphuric acid, and undertake the following steps:(i) 4.805 g of solid sodium tetraborate (Na2B4O7) are added to a 250 mL volumetric flask, and the solution made up to the mark with distilled water.(ii) 25.00 mL aliquots of the stock solution from (i) are transferred to conical flasks, for titration against the sulphuric acid solution in the burette.(iii) You perform titrations using two different indicators: bromocresol green, and phenolphthalein.With bromocresol green, the average titre volume is 22.50 cm3, while with phenolphthalein, the average volume is 9.50 cm3.(a) Write the balanced equation for the reaction between Na2B4O7 and sulphuric acid
A. CaSO4 B. Ba3(PO4)2 C. PbS D. Pb3(PO4)2 Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine thatcobalt(II) carbonate is more soluble than _______, and cobalt(II) carbonate is less soluble than _______ It is not possible to determine whether cobalt(II) carbonate is more or less soluble than _________ by simply comparing Kspvalues.
Consider these compounds: A. Ba3(PO4)2 B. Ca3(PO4)2 C. PbCrO4 D. CaCrO4 Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine that barium sulfite is more soluble than fill in the blank 1, and barium sulfite is less soluble than fill in the blank 2. It is not possible to determine whether barium sulfite is more or less soluble than fill in the blank 3 by simply comparing Ksp values.
On the basis of the general solubility rules given in Table 7.1 and the ones that are on the handout I gave to you in class, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate why (which rules apply). Hint: Write the reaction down and determine what the products will be. And then, you can use the solubility rules I gave out in class and are also in Table 7.1 of your textbook. a. iron(III) chloride, FeCl3, and phosphoric acid, H3PO4 b. barium nitrate, Ba(NO3)2, and sodium sulfate, Na2SO4 c. potassium chloride, KCl, and iron(II) sulfate, FeS
Write the balanced COMPLETE ionic equation for the reaction when ammonium carbonate and calcium chloride are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
A patient had severe acid reflux symptoms and decided to take the antacid, Amphojel (aluminum hydroxide). What is another typical, everyday name for an acid-base reaction? How many grams of aluminum hydroxide are required to produce 4.27 moles of water? If this is also an oxidation-reduction (redox) and/or precipitation reaction, then show work to support your answer. If this is not an oxidation-reduction (redox) and/or precipitation reaction, then show work to support your answer.
Dissociation of the following equation in water (equation should be balanced and with state symbols) Sulfuric acid, Nitric acid, Oxalic acid, Phosphoric acid, Ethanoic acid eg HCL(aq) + H₂O(I)⇌H₃O⁺(aq)+Cl?(aq) would prefer if text and symbols were properly aligned like above and in text format
Write the balanced NET ionic equation for the reaction when Pb(NO₃)₂ and KI are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
Ima Kemist is analyzing a solution of kansui (potassium carbonate) by precipitating the carbonate with Epsom salt (magnesium sulfate).a. Write the balanced molecular and net ionic equations for the reaction between aqueous potassium carbonate and aqueous magnesium sulfate. Include states of matter.b. Ima weighs a coffee filter and filters out the precipitate formed from her experiment. She allows the filter and precipitate to dry, then weighs the filter and precipitate, calculating the mass of precipitate by difference. However, the filter and precipitate were not completely dry. Is the mass Ima calculated higher than, lower than, or equal to the true mass of the precipitate?c. Ima uses the mass of the wet precipitate to calculate the concentration of potassium carbonate. Is this calculated concentration higher than, lower than, or equal to the true concentration of the sample?
For the reaction below, fill in the missing phases in the parentheses, balance the reaction and then write out a net ionic equation for the reaction