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In the tetrathionate ion (S4O6)2-, the total charge of the ion is 2-. Each oxygen atom has an oxidation number of -2, totaling -12 for all six oxygen atoms. Since the overall charge is 2-, the sum of the oxidation numbers of sulfur atoms must equal +2. With four sulfur atoms present, each sulfur atom in the tetrathionate ion has an oxidation number of +6.
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What is the oxidation number for BaSO4?
The oxidation number for BaSO4 is 6. It goes as follows: +2 for Ba +6 for S -2 for O
What is the product when thiosulfate ions and iodine react?
2 S2O32- + I2 --> S4O62- + 2 I-thiosulfate + iodine -> tetrathionate* + iodide* -O3=-=S-S-S-S=-=O3-
What part of an ion's symbol indicates it's charge?
The number represents the charge on the ion. The number is the quantity of electrons lost or gained by the elemental atom to become an ion. Thus gaining 1 electron makes the ion -1, because the electron is negatively charged. Losing an electron results in a positively charged ion +1. So if two electrons are gained the charge is -2. These numbers are also called oxidation numbers, representing the oxidation state of the element as the ion.
Does potassium iodide react with sodium carbonate?
Yes, potassium iodide would react with sodium carbonate to form potassium carbonate and sodium iodide. This reaction is a double displacement reaction where the cations and anions are exchanged between the compounds.
Redox titration using sodium thiosulphate and potassium iodate?
In redox titration using sodium thiosulfate and potassium iodate, the iodate ion (IO3-) is reduced to iodine (I2) by thiosulfate ion (S2O32-). The iodine formed is then titrated with sodium thiosulfate until the endpoint is reached, indicated by a color change from yellow to colorless when all the iodine is reacted. This method is commonly used to determine the concentration of oxidizing agents in a sample.
What is the oxidation number for BaSO4?
The oxidation number for BaSO4 is 6. It goes as follows: +2 for Ba +6 for S -2 for O
What is the product when thiosulfate ions and iodine react?
2 S2O32- + I2 --> S4O62- + 2 I-thiosulfate + iodine -> tetrathionate* + iodide* -O3=-=S-S-S-S=-=O3-
Balancing and after balancing?
s2o32-to give s4o62-
What part of an ion's symbol indicates it's charge?
The number represents the charge on the ion. The number is the quantity of electrons lost or gained by the elemental atom to become an ion. Thus gaining 1 electron makes the ion -1, because the electron is negatively charged. Losing an electron results in a positively charged ion +1. So if two electrons are gained the charge is -2. These numbers are also called oxidation numbers, representing the oxidation state of the element as the ion.
What will happen when bromine reacts with sodium thiosulphate?
When bromine reacts with sodium thiosulfate, the bromine will oxidize the thiosulfate ion to form sulfate ions and release bromide ions. This reaction can be used as a redox titration method to determine the concentration of bromine in a solution.
What is the balanced chemical equation for the reaction between hypochlorite ion and thiosulfate ion?
The balanced chemical equation for the reaction between hypochlorite ion (OCl-) and thiosulfate ion (S2O3^2-) is: 2OCl- + 2S2O3^2- -> 2Cl- + S4O6^2- + 2OH-
Does potassium iodide react with sodium carbonate?
Yes, potassium iodide would react with sodium carbonate to form potassium carbonate and sodium iodide. This reaction is a double displacement reaction where the cations and anions are exchanged between the compounds.
Given that 31.6ml of 0.141M Na2S2O3 is needed to reach the stoichiometric point how many grams of Cl2 are in the titrated?
Thiosulfate: 2 S2O32- --> S4O62- + 2e-equivalency to:Chlorine: 1 Cl2 + 2e- --> 2Cl-31.6 ml * 0.141 mmol/ml S2O32- = 4.456 mmol S2O32-= 4.456 *(2 electron / 2 S2O32-) = 4.456 mmol (electrons) == 4.456 *(1 Cl2 / 2 electron) = 2.228 mmol Cl2 == 2.228 * 70.90 mg/mmol Cl2 = 158 mg == 0.158 g Chlorine
Redox titration using sodium thiosulphate and potassium iodate?
In redox titration using sodium thiosulfate and potassium iodate, the iodate ion (IO3-) is reduced to iodine (I2) by thiosulfate ion (S2O32-). The iodine formed is then titrated with sodium thiosulfate until the endpoint is reached, indicated by a color change from yellow to colorless when all the iodine is reacted. This method is commonly used to determine the concentration of oxidizing agents in a sample.
Equation between potassium iodate and sodium thiosulphate?
The equation between potassium iodate (KIO3) and sodium thiosulfate (Na2S2O3) involves a redox reaction. In the presence of an acid, potassium iodate is reduced to iodine (I2), while sodium thiosulfate is oxidized to form sodium tetrathionate (Na2S4O6). The balanced chemical equation for this reaction is 5Na2S2O3 + 2KIO3 + 8HCl → 5Na2S4O6 + 2I2 + 2KCl + 6H2O.
What are the five different chemical reactions?
The large diversity of chemical reactions and approaches to their study results in the existence of several concurring, often overlapping, ways of classifying them. Below are examples of widely used terms for describing common kinds of reactions.Isomerisation, in which a chemical compound undergoes a structural rearrangement without any change in its net atomic composition; see stereoisomerismDirect combination or synthesis, in which 2 or more chemical elements or compounds unite to form a more complex product:N2 + 3 H2 → 2 NH3 Chemical decomposition or analysis, in which a compound is decomposed into smaller compounds or elements:2 H2O → 2 H2 + O2 Single displacement or substitution, characterized by an element being displaced out of a compound by a more reactive element:2 Na(s) + 2 HCl(aq) → 2 NaCl(aq) + H2(g) Metathesis or Double displacement reaction, in which two compounds exchange ions or bonds to form different compounds:NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s) Acid-base reactions, broadly characterized as reactions between an acid and a base, can have different definitions depending on the acid-base concept employed. Some of the most common are: Arrhenius definition: Acids dissociate in water releasing H3O+ ions; bases dissociate in water releasing OH- ions.Brønsted-Lowry definition: Acids are proton (H+) donors; bases are proton acceptors. Includes the Arrhenius definition.Lewis definition: Acids are electron-pair acceptors; bases are electron-pair donors. Includes the Brønsted-Lowry definition.Redox reactions, in which changes in oxidation numbers of atoms in involved species occur. Those reactions can often be interpreted as transferences of electrons between different molecular sites or species. An example of a redox reaction is:2 S2O32−(aq) + I2(aq) → S4O62−(aq) + 2 I−(aq) In which I2 is reduced to I- and S2O32- (thiosulfate anion) is oxidized to S4O62-. Combustion, a kind of redox reaction in which any combustible substance combines with an oxidizing element, usually oxygen, to generate heat and form oxidized products. The term combustion is usually used for only large-scale oxidation of whole molecules, i.e. a controlled oxidation of a single functional group is not combustion.C10H8+ 12 O2 → 10 CO2 + 4 H2O CH2S + 6 F2 → CF4 + 2 HF + SF6 Disproportionation with one reactant forming two distinct products varying in oxidation state.2 Sn2+ → Sn + Sn4+ Organic reactions encompass a wide assortment of reactions involving compounds which have carbon as the main element in their molecular structure. The reactions in which an organic compound may take part are largely defined by its functional groups.
What are the five chemical reactions?
The large diversity of chemical reactions and approaches to their study results in the existence of several concurring, often overlapping, ways of classifying them. Below are examples of widely used terms for describing common kinds of reactions.Isomerisation, in which a chemical compound undergoes a structural rearrangement without any change in its net atomic composition; see stereoisomerismDirect combination or synthesis, in which 2 or more chemical elements or compounds unite to form a more complex product:N2 + 3 H2 → 2 NH3 Chemical decomposition or analysis, in which a compound is decomposed into smaller compounds or elements:2 H2O → 2 H2 + O2 Single displacement or substitution, characterized by an element being displaced out of a compound by a more reactive element:2 Na(s) + 2 HCl(aq) → 2 NaCl(aq) + H2(g) Metathesis or Double displacement reaction, in which two compounds exchange ions or bonds to form different compounds:NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s) Acid-base reactions, broadly characterized as reactions between an acid and a base, can have different definitions depending on the acid-base concept employed. Some of the most common are: Arrhenius definition: Acids dissociate in water releasing H3O+ ions; bases dissociate in water releasing OH- ions.Brønsted-Lowry definition: Acids are proton (H+) donors; bases are proton acceptors. Includes the Arrhenius definition.Lewis definition: Acids are electron-pair acceptors; bases are electron-pair donors. Includes the Brønsted-Lowry definition.Redox reactions, in which changes in oxidation numbers of atoms in involved species occur. Those reactions can often be interpreted as transferences of electrons between different molecular sites or species. An example of a redox reaction is:2 S2O32−(aq) + I2(aq) → S4O62−(aq) + 2 I−(aq) In which I2 is reduced to I- and S2O32- (thiosulfate anion) is oxidized to S4O62-. Combustion, a kind of redox reaction in which any combustible substance combines with an oxidizing element, usually oxygen, to generate heat and form oxidized products. The term combustion is usually used for only large-scale oxidation of whole molecules, i.e. a controlled oxidation of a single functional group is not combustion.C10H8+ 12 O2 → 10 CO2 + 4 H2O CH2S + 6 F2 → CF4 + 2 HF + SF6 Disproportionation with one reactant forming two distinct products varying in oxidation state.2 Sn2+ → Sn + Sn4+ Organic reactions encompass a wide assortment of reactions involving compounds which have carbon as the main element in their molecular structure. The reactions in which an organic compound may take part are largely defined by its functional groups.
