Which of the following statements are correct? K2CrO4 is used as an indicator in the argentometric titration Eosin is used as an indicator in the thiocyanometric titration K2Cr2O7 is used as an indicator in the argentometric titration Eosin is used as an indicator in the

Q: The iodate ion has a number of insoluble compounds. The Ksp for AglO3 is 3.0 x 10-8 and the Ksp for…

A: To find the solubility of La(IO3)3 in a 0.115 M solution of NaIO3, we need to use the solubility…

Q: buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00…

A: We will calculate pKa using henderson hasselbalch equation.

Q: why does this happen? After the sodium oxalate was added to the lead nitrate, a white precipitate…

A: Your observations are related to a chemical reaction involving sodium oxalate and lead nitrate.…

Q: I have a 3 step problem about Determination of an Equilbrium constant.

A: Step – 1: The initial moles of given Fe3+ and SCN- ions are determined as follows,

Q: mount of X used in titration: 100.0 mmol amount NaOH added (mmol) (b) 35.0 220.0 (c) pH 2.558 4.482…

A: We have following formula -  pH = pKa + log [A-]/[HA]    Then -  (a)  pH = pKa + log [A-]/[HA]…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: Given : moles of Ca(OH)2 present = 0.00333 mol And volume of Ca(OH)2 solution = 50.0 mL

Q: Can you explain the problem?

A: Step 1: Step 2: Step 3: Step 4:

Q: What volume of 0.130 M  KMnO4 would be required to titrate 0.36 g  of  K2[Cu(C2O4)2]⋅2H2O

A: We should equal equivalent of both KMnO4 and compund ion to get volume of KMnO4 Equivalent =…

Q: The plot below is for the titration of 30.00 mL CH3COOH with 0.150M KOH: CH3COOH (aq) + KOH(aq) →…

A: Given: VCH3COOH = 30.0 ml , MKOH = 0.150 MVKOH = 38.2 ml (at the equivalence point from the given…

Q: A 0.1064-g of aldrin pesticide sample was decomposed and the liberated chloride was extracted using…

A:

Q: Taking into account the effect of activity, calculate the pH of each of the following: 1. 0.10 M…

A: Since you have asked a question with multiple subparts we will answer the first three subparts for…

Q: If the system CaCO3(s) + 2H+(aq) --> Ca2+(aq) + CO2(g) + H2O(l) is saturated with respect to CaCO3,…

A: In the system, CaCO3(s) + 2H+(aq) --> Ca2+(aq) + CO2(g) + H2O(l) we can see that H+ is reacting…

Q: The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+,…

A: we have to calculate the value of pCu2+

Q: Calculate the molar solubility of aluminum hydroxide, Al(OH),, in a solution buffered at pH 12.00 Kp…

A:

Q: Curved arrows are used to illustrate the flow of electrons. Follow the arrows to predict the product…

A: Given reaction :

Q: For each of the following compounds, decide whether the compound's solubility in aqueous solution…

A: To determine whether the solubility of a compound changes with pH, we need to consider the effect of…

Q: A solution of phosphoric acid (H3PO4) with a known concentration of 0.250 M H3PO4 is titrated with a…

A: At third equivalence point, all the  H3PO4 molecule get converted to PO4-3 i.e complete…

Q: What will be the pH if 5.00 grams of solid KOH is added to 500 mL of a solution containing 0.020…

A: Since you have posted 2 completely unrelated questions, we are entitled to answer only the first.

Q: Indicator Measurement Colour of Indicator phenol red pOH = 6.8     Indicator Measurement Colour of…

A:

Q: Which Titrations go with which graph?

A:

Q: Explain why K2CrO4 is used as an indicator in Argentometric titration

A: Argentometric titration is the titration method, which is used for the detection of halides or…

Q: Ethyl orange, an indicator, has a Ka of 2.0 x 10–4. The protonated form is red and the deprotonated…

A: ethyl orange is a pH indicator frequently used in titration because of its clear and distinct color…

Q: A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN. If the K+ for Cu(CN)4²- is 1.0 × 1025,…

A: Initial concentration of Cu2+ = 2.2 × 10-3 MInitial concentration of LiCN = 0.33 MFormation…

Q: Given the values of Ka and Kh below, which of the systems given would be most suitable to use to…

A: The pH of a buffer solution remain close to the pKa value of its acid in weak acid / base and its…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.