Wgat is the [OH-] of a bleach sample that registers 11.41 on a pH meter?

Q: The [ H3O+] of a solution with pH = 5.60 is Group of answer choices 3 × 10-6 M. 2.5 × 10-8 M.…

A: Given, pH = 5.60.

Q: How many milliliters of 0.105 M HCl are needed to titrate 45 mL of 9.50 x 10-2 M NaOH?

A: The equation is, M1V1 = M2V2 M1 = Molarity of HCl V1 = Volume of HCl M2 = Molarity of  NaOH V2 =…

Q: 14. Which indicator in yellow in a solution with a pH of 987 A methyl ornge R. hromthymol Mue C…

A: We have to tell which option is correct

Q: Determine the concentration of a solution of ammonium chloride (NH4Cl) that has pH of 5.37at 25C.…

A:

Q: Which of the following dissociations will increase the pH scale significantly? Select one: O a.…

A: pH scale is high when the basicity increases that is the concentration of the hydroxy ions…

Q: Which of the following compunds is a weak acid? a) Phenol b) cyclohexanol c) ethanol d)…

A: Hello. Since you have posted multiple questions and not specified which question needs to be solved,…

Q: 4. At 40.°C the value of Kw is 2.92 x 10-14. a. Calculate the [H*] and [OH] in pure water at 40.°C.…

A: Since you have asked multiparts questions, we will solve the first three sub parts questions for…

Q: -3 The pH value of a (0.062 + 0.002) mol dm HCI solution is: Select one: 1.21 0.11 1.21 1 1.21 0.01…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: 9 Question 10 - Ch 19 HW - Conne X b Answered: Find the pH of the equ b Success Confirmation of…

A:

Q: 5- Instrumental methods of analysis example such 6- Acid equivalent weight can calculated by…

A: Fill in the blanks are given as:

Q: Show your work, use general chemistry rules for significant figures. 2. The pH of a solution made…

A: pOH = 14 - pH pOH = pKb + log[salt]/[base]

Q: Calculate (OH ] and pH for each of the following solutions. (a) 0.0083 M NaOH [OH"] = 2.081 X M pH =…

A: pOH  = -log [OH-] pH + pOH = 14  pH = 14- pOH

Q: 3- The concentration of a solution containing 5 ng of KCI in 200 mg water is : (0.025 ppt, 0.025…

A: 3) We have given Mass of KCl = 5 ng = 5×10-9 g Mass of water = 200 mg = 200×10-3 g   Therefore…

Q: 100 ml of base was streaked with different volumes of acid (equal concentrations) and the following…

A:

Q: Calculate the volume of NaOH 0.50M needed to obtain a 1:1 acid:acetate ratio from 50mL of acetic…

A: Given,  The volume of 0.50 M NaOH needed to obtain 1:1 acid:acetate ratio from 50mL of 0.20 M acetic…

Q: If the pKa of the indicator is approximately 6, to which of the following equivalence point will it…

A: Given, pKa = 6 At equivalence point,  pH = ?

Q: Which one of the multiple choice is correct? 1. What is the percent composition(by mass) of…

A: "Since, you have posted multiple questions, we will solve only first question for you as per the…

Q: Draw a pC-pH diagram for a monoprotic acid with a Ka = 10-3 M and CTA = 10-2.5 M. %3D %3D At what pH…

A: A pC-pH diagram depicts a line representing the variation of concentration of hydroxide ion as a…

Q: Dilution. 100 mL100 mL of a solution of hydrochloric acid with pH 5.0 pH 5.0 is diluted to 1 L1 L.…

A: pH of a solution is equal to the negative logarithm of hydrogen ion concentration. Using this…

Q: Why are buffer solutions of increasingly higher pH used to elute the column that generates the…

A: The reason is as given below:

Q: at 95 ℃ water has an autoionization constant (Kw) of 4.518 X 10-13. Determine the ph of pure water…

A: Given :- Kw at 95°C = 4.518 × 10-13  To determine :- pH of pure water at 95°C

Q: what is the Ka value

A:

Q: Ka for nitrouse acid ,HNO2 is 4.5 x10^-4.what is the value of Kb for the nitrite ion NO2^-

A: Conjugate acid-base pair is a pair which differ by only one proton.

Q: Calculate the concentrations of hydronium ion and hydroxide ion at 25°C in: a. 0.12 MHNO; [H;O"]= M…

A:

Q: Calculate the pH of 0.7 M of Aniline solution CeHgNH2 CeHgNH2 + H20 CeHgNH3 + OH K for Aniline = 4…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: The pH of a 1.5 M solution of 4-chlorobutanoic acid (HC H,0,Cl) is measured to be 2.17. 4 6. 2.…

A:

Q: (b) 0.15 moldm of benzoic acid (CeHsCOOH; Ka of benzoic acid = 6.3 x 10-5 moldm- %3D 3)

A: Acid dissociation constant measures the acidic strength of an acid. Higher the value of Ka, higher…

Q: If the pH level of a fluid is 8.4, what is [H+] for the fluid? Give exact and approximate answers

A:

Q: What are the advantages and disadvantages of 4.5-7.5 pH paper?

A: pH paper is of following types: 0-14 pH paper: This paper can measure a pH varying from 0 pH value…

Q: The pH of 30.0 mL of 0.80 M Benzoic acid (Ka = 5.6 x 10-5) is _____________ (with 3 significant…

A: There are two types of types of acids/bases. Strong acids and strong bases are those acids and bases…

Q: he pH of the solution formed by mixing 50 ml of 0.1 M CH3COOH solution (Ka = 1.8 × 10-⁵) with 45 ml…

A: Answer :-  (b) 5.7  The pH of the solution formed by mixing 50 ml of 0.1 M CH3COOH solution (Ka =…

Q: Determine the pH of a solution made of 0.0082M H3PO4 and 0.0046M Na2HPO4. (Ka of H3PO4 = 7.11 x…

A: Balance chemical equation:                                   H3PO4 + Na2HPO4  ----->   2NaH2PO4…

Q: A solution of dimethylamine is prepared by dissolving 1.3525 grams of dimethylamine in 25 mL ethanol…

A: Dimethylamine reacts with HCl as: CH3NHCH3+HCl→CH3NH2+CH3+Cl-

Q: A solution of lactic acid, HC3H5O3, on a laboratory shelf was of undetermined concentration. If the…

A:

Q: What is the pH of 100.0 mL of 0.10 M HNO;? nooulos M 005.0s ai nois 01 x 02.1 g CH'COOH What is the…

A: pH = -log [H+]

Q: Determine the Ka value [H +]eq Solution 5  4.68 X 10-10 M Directions Take a 30.0 mL sample…

A: The concentration of hydroxyl ion is calculated as follows:

Q: What is the pH of 0.0050 M NH3 (Kb = 1.8 x 10-5) 10.48 3.52 11.70 2.30

A: Given that the concentration of NH3 is 0.0050 M. NH3 is a weak base and the concentration of…

Q: Calculate H30| of the following polyprotic acid solution: 0.130 M H2CO3 (Kal = 4.3 x 10 7, K2 = 5.6…

A:

Q: What is the ph of 0.750M lactic acid? And show the ICE table

A: pH of 0.750 lactic acid can be calculated as follows

Q: The value of Kw at 40 °C is 2.92 x 10-14 a. Calculate the [H*] and [OH] in pure water at 40 °C. b.…

A: Calculations (a) Given Kw = 2.92 x 10-14 [H3O+] [OH-] = 2.92 x 10-14 Since the solution is neutral…

Q: At 40 °C the value of Kw is 2.92 x 10-14. Calculate the [H+] and [OH-] in pure water at 40 °C. What…

A: H2O ⇋ H+ + OH- Kw=[H+][OH-] [H+]=[OH-]=x 2.92×10-14=x2 x=1.7×10-7=[H+]=[OH-]

Q: 1. Calculate what pH should be for Mg2+ at 1.31 x 10-2 concentration. (Mg(OH)2(s) Mg2+ (aq) +…

A:

Q: What mass of NaN3 needs to be added to water to give a 1.0 L solution with pH= 9.43. For HN3 : Ka =…

A:

Q: Calculate the pH of a solution of 0.01 M NaF, given Kb for F- = 1.4 x 01-11. Group of answer…

A: NaF <---> Na+ + F-  ICE Table –       F-   +     H2O <---> HF    +    OH- I   0.01…

Q: What is the pH of 0.541 M dimethylammonium iodide, (CH3)2NH21? At 25°C, the Kb of (CH3)2NH is 5.9 x…

A: Dimethylammonium iodide is a salt of a strong acid, HI, and weak base, (CH3)2NH. So, in this case,…

Q: How many milligrams of CH3COOH (fw 60) should be added to 250 mL of water to get pH 3. K. = 1 x 10-5

A: CH3COOH is weak acid in aqueous solution. It will dissociate in solution as below-

Q: Calculate the pH of the following mixture 500 ml 0.35 M CH3CH2NH2 + 500 ml 0.25 M HNO3

A: Given : The volume of CH3CH2NH2= 500 ml Molarity of CH3CH2NH2 =0.35 M The volume of HNO3=500 ml…

Q: Formic acid (HCOOH) has a Ka = 1.8 × 10-4. What is the pH of a 25.00mL sample of 0.205 M formic…

A: Given: Ka = 1.8 × 10-4 [HCOOH] = 0.205 M

Q: I have ammonia (20 M) dissociating in water. What is the pH? (4 sig figs). Kb= 1.8x 10-5

A: Ammonia disassociates in water to form Ammonium ion and Hydroxide ion NH3 + H2O <---> NH4+ +…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.