A solution of potassium chloride when mixed with silver nitrate

[ "article:topic", "solubility", "strong acid", "strong base", "weak acid", "acid", "Acid-base reaction", "base", "insoluble", "neutralization reaction", "precipitate", "Precipitation reaction", "reducing agent", "salt", "soluble", "weak base", "showtoc:yes", "license:ccby", "source-chem-167334", "source-chem-167675" ] \( \newcommand\) • • • Precipitation Reactions and Solubility Rules A precipitation reaction is one in which dissolved substances react to form one (or more) solid products. Many reactions of this type involve the exchange of ions between ionic compounds in aqueous solution and are sometimes referred to as double displacement, double replacement, or metathesis reactions. These reactions are common in nature and are responsible for the formation of coral reefs in ocean waters and kidney stones in animals. They are used widely in industry for production of a number of commodity and specialty chemicals. Precipitation reactions also play a central role in many chemical analysis techniques, including spot tests used to identify metal ions and gravimetric methods for determining the composition of matter (see the last module of this chapter). The extent to which a substance may be dissolved in water, or any solvent, is quantitatively expressed as its solubility, defined as the maximum concentration of a substance that can be achieved under specified conditions. Substances with relatively large solubilities are said to be soluble. A substance will precipitate when ...

Part A What mass of silver chloride can be produced from 1.19L of a 0.293M solution of silver nitrate? Express your answer with the appropriate units. mass of AgCl = Part B The reaction described in Part A required 3.47L of potassium chloride. What is the concentration of this potassium chloride solution? Express your answer with the appropriate units. ¢ € £ ¥ ‰ µ · • § ¶ ß ‹ › « » ≤ ≥ – — ¯ ‾ ¤ ¦ ¨ ¡ ¿ ˆ ˜ ° − ± ÷ ⁄ × ƒ ∫ ∑ ∞ √ ∼ ≅ ≈ ≠ ≡ ∈ ∉ ∋ ∏ ∧ ∨ ¬ ∩ ∪ ∂ ∀ ∃ ∅ ∇ ∗ ∝ ∠ ´ ¸ ª º † ‡ À Á Â Ã Ä Å Æ Ç È É Ê Ë Ì Í Î Ï Ð Ñ Ò Ó Ô Õ Ö Ø Œ Š Ù Ú Û Ü Ý Ÿ Þ à á â ã ä å æ ç è é ê ë ì í î ï ð ñ ò ó ô õ ö ø œ š ù ú û ü ý þ ÿ Α Β Γ Δ Ε Ζ Η Θ Ι Κ Λ Μ Ν Ξ Ο Π Ρ Σ Τ Υ Φ Χ Ψ Ω α β γ δ ε ζ η θ ι κ λ μ ν ξ ο π ρ ς σ τ υ φ χ ψ ω ℵ ϖ ℜ ϒ ℘ ℑ ← ↑ → ↓ ↔ ↵ ⇐ ⇑ ⇒ ⇓ ⇔ ∴ ⊂ ⊃ ⊄ ⊆ ⊇ ⊕ ⊗ ⊥ ⋅ ⌈ ⌉ ⌊ ⌋ 〈 〉 ◊ RELATED QUESTIONS if 5.67 moles of Fe were produced, how many moles of CO2 would be produced? Answers · 1 i need help with stoichemtry Li3N+3H2O-->NH3+3LiOH Answers · 1 How many grams of water will be produced from 32 grams of oxygen gas Answers · 2 what's the easiest way to balance chemical equations? Answers · 1 Can someone please check my work and answers on these two titration problems? Answers · 1 RECOMMENDED TUTORS

• • • • Question:84. Silver can be precipitated from a silver nitrate solution with potassium chloride. Write a balanced equation for the reaction and determine the mass of potassium chloride required to precipitate all of the silver in 1.00 L of a 0.500M silver nitrate solution. 90. An acid solution is 0.100M in HC volume of a 0.150MKOH solutior all the acld in 500.0ml of 84. Silver can be precipitated from a silver nitrate solution with potassium chloride. Write a balanced equation for the reaction and determine the mass of potassium chloride required to precipitate all of the silver in 1.00 L of a 0.500 M silver nitrate solution. 90. An acid solution is 0.100 M in HC volume of a 0.150 M KOH solutior all the acld in 500.0 ml of this 90 81. Find the mass of barium metal O 2 ​ to produce enough barium os solution of OH. (Hint Barlum Previous question Next question

Table of Contents • • • • • • • • What happens when potassium chloride reacts with silver nitrate? When an aqueous solution of potassium chloride(KCl) when mixed with silver nitrate(AgNO3) solution an insoluble white substance formed is silver chloride(AgCl). The chemical reaction are as follows : KCl(aq) + AgNO3(aq) → KNO3(aq) + AgCl (s). It is an example of double displacement reaction. What happens when you add silver nitrate to chlorine? When a few drops of a silver nitrate solution are added to a slightly acidic aqueous solution that contains chloride ions, a white precipitate of silver chloride will form. What happens when potassium and chlorine are combined? Potassium forms ions with a positive charge. A compound is formed when potassium reacts with chlorine, which forms ions with a negative charge. This electron is transferred to a chlorine atom to form a chloride ion. In KCl, both ions have full outer energy levels (noble gas configuration). When solutions of silver nitrate and potassium chloride are mixed a white precipitate forms? Complete answer: Silver chloride (AgCl) is formed as an insoluble white precipitate when aqueous solution of potassium chloride (KCl) and silver nitrate (\[AgN\)) and a white precipitate is formed. What is the solution of potassium chloride? Potassium chloride (KCl, or potassium salt) is a metal halide salt composed of potassium and chlorine. It is odorless and has a white or colorless vitreous crystal appearance. The solid dissolves r...

Video Transcript When we mix silver nitrate and potassium chloride together, a white precipitate of silver chloride forms. Calculate the mass of potassium chloride when two grams of silver chloride is precipitated. Give your answer to two decimal places. The molar mass of silver is 108 grams per mole, potassium is 39 grams per mole, and chlorine is 35.5 grams per mole. In this question, we are asked to determine the mass of potassium chloride in a solution that reacted when given the mass of a silver chloride precipitate. This is an example of precipitation gravimetry, which is an analytical technique that uses the formation and mass of a precipitate to determine the mass of an analyte. In this problem, the precipitate is silver chloride and the analyte is potassium chloride. Before we can calculate the mass of potassium chloride, we need to write a balanced equation for the precipitation reaction. Silver nitrate, or AgNO3, reacts with potassium chloride, or KCl. And one of the products of the reaction is the silver chloride precipitate, or AgCl. Based on the equation that we have so far, we have not included the potassium or nitrate ions in the products. Therefore, the missing product is potassium nitrate, or KNO3, which remains dissolved in the solution after the reaction. After counting up the number of each type of atom on either side of the equation, we notice that the chemical equation is already balanced. We now know that the molar ratio of potassium chloride to sil...

This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. See Answer See Answer See Answer done loading Question:When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation AgNO, (aq) + KCl(aq) - AgCl(s) + KNO, (aq) Part A What mass of silver chloride can be produced from 1.93 L of a 0.217 M solution of silver nitrato? Express your answer with the appropriate units. View Available Hint(s) HA When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation AgNO, (aq) + KCl(aq) - AgCl(s) + KNO, (aq) Part A What mass of silver chloride can be produced from 1.93 L of a 0.217 M solution of silver nitrato? Express your answer with the appropriate units. View Available Hint(s) HA ? mass of AgCI Value Units Submit Part B The reaction described in Part A required 3.80 L of potassium chloride. What is the concentration of this potassium chloride solution? Express your answer with the appropriate units. View Available Hint(s) 0 ? Symbols Previous question Next question

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