## What Is The Ph Of A 0.050 M Lioh Solution?

The answer is: e. **12.70** pOH = -log[OH-] = -log[LiOH] =…Jan 28 2021

## What is the pH of a LiOH solution?

The LiOH concentrations and room temperature pH values are respectively: 0.06M LiOH pH 12.8 0.1M LiOH pH 13.1 0.5M LiOH pH 13.6 0.85M LiOH pH **13.8** 1.0M LiOH pH 14.0 [8].

## What is the pH of a 0.25 M solution of LiOH?

**PH = 13.40**and [OH-] = 0.50 M Ob.PH = 0.600 and (OH”]=0.50 M OC.

## What is the pH of 0.01 M solution of LiOH?

So to get back and forth between pH and pOH just note that the two numbers have to equal 14. So if the pH of 0.1 M HCl is 1 then the pOH = 14 – 1 = 13 • and if the pOH of 0.01 M LiOH = 2 then the pH **= 14 -2 = 12**.

## What is the pH of a .0025 M solution?

Mike Schuck · Ernest Z. The pH is **1.60**.

## What is the pH of 0.001 m h2so4?

The pH of 0.01 M sulphuric acid is **1.699**.

## What is the pH of lithium?

Hydrolysis of lithium carbonate produces basic solutions by generating lithium hydroxide and lithium hydrogen carbonate. The pH values can be calculated based on pKa values. The pH of a 0.02 mol solution is calculated to be **11.3**.

## What is the pH of a 0.056 M hno3 solution?

**1.25**. Okay that’s the Ph.

## What is the pH of a 0.0001 m HCl solution?

The pH and pOH of 0.0001 M HCl solution are **4 and 10** respectively.

## How do you find the pH of 0.05 m H2SO4?

∴pH of 0.05M of H2SO4 is **1**.

## What is the pH of a 0.0025 m NaOH solution?

**12.40**.

## What is the pH of a 0.02 M solution of KOH?

pH=14−(1.57)=**12.4** .

## What is the pH of a 0.00125 M HCl solution?

**11.1**.

## What is the pH of a 0.045 M HCl solution?

The solution with [H^{+}] = 0.0045 M will have a pH of **2.35**.

## What is the pH of a 0.10 M solution of KOH?

If concentration of KOH is 0.1 M pH value may be **13**. If concentation is 0.0001 M pH value will be 10.

## What is the pH of a 3m solution of hno3?

**1.6021**.

## How do you find the pH of a H2SO4 solution?

**pH = -log**

_{10}[H^{+}(aq)]**pH = -log**

_{10}[c + x]…

Example: Calculating pH of Sulfuric Acid using R.I.C.E. Table and Quadratic Equation.

K_{a2} |
= | [H^{+}(aq)][SO_{4}^{2}^{–}(aq)] [HSO_{4}^{–}(aq)] |
---|---|---|

x^{2} + 0.5x + 1.2 × 10^{–}^{2}x – 6.0 × 10^{–}^{3} |
= | |

x^{2} + 0.512x – 6.0 × 10^{–}^{3} |
= |

## How do you find the pH of 0.01 m H2SO4?

**pH= -log**(H+) Here H+ refers to the concentration of H+ ions or the Hydronium ions. Here it can be clearly observed that 1 moles of sulphuric acid gives rise to 2 moles of H+ ions. which is equal to 1.698. Therefore pH of 0.01 moles of H2SO4 is 1.698 or 1.70.

## What is the pH of a 0.02 M solution of sulfuric acid H2SO4?

The pH of 0.02 M is **1.4**.

## Is Lithium acidic or basic?

Lithium carbonate is somewhat toxic. It is **a base** and reacts with strong acids.

## How do you find the pH of a solution?

To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter (molarity). The pH is then calculated using the expression: **pH = – log [H _{3}O^{+}].**

## Does LiOH contain H+?

…

The chemical formula for lithium hydroxide is LiOH.

LiOH | Lithium hydroxide |
---|---|

Lithium hydroxide Chemical Formula | LiOH |

## What is the pH of a 0.00010 M solution of hno3?

Explanation: log10{0.0001} = log10(10−4)=−4 by definition of the log function. Thus pH **= 4** and necessarily pOH=10 .

## What is the pH of a 0.014 M Ca OH 2 solution?

Question: what is the pH of a 0.014 M Ca(OH)2 solution? the answer is supposed to be **12.45** but i keep getting12.

## Is a solution with a pH of 8.5 acidic or basic?

_{2}.) Pure water with a pH of 7 is neutral. With a pH of less than 7 wine is acidic.

…

Example 12.

Substance | pH |
---|---|

blood | 7.4 |

seawater |
8.5 |

milk of magnesia | 10.5 |

ammonia solution | 12.5 |

## What is the H+ ion concentration of 0.001 M HCl?

When you see [H+] it should be read as “the Molar concentration of hydrogen ions”. This means “The molar concentrations of HCl and its dissociated hydrogen ions are both equal to 0.001 M.” Using scientific notation to get a power of ten **[H+] = 1 x 10-3 M**.

## What is the pH of a 0.050 M solution of H2SO4 Ka2 0.012 )?

**1.23**.

## What is the normality of 0.05 m H2SO4?

Since 2 protons are available to react on each molecule of H2SO4 the normality is **2 N**.

## How do you make 0.05 M sulfuric acid?

Thus you might make 0.5 M H2SO4 by diluting 27.2 ml concentrated H2SO4 to a final volume of 1 L and then **diluting this solution 1:100 (10 ml diluted to a final volume of 1000 ml)** to obtain 0.05 M H2SO4.

## What is the pH of a 0.100 M NaOH solution?

**13**.

## What is the pH of a 1.50 M aqueous solution of sodium hydroxide NaOH )?

The pH of your NaOH solution is **13**.

## What is the pH of 1M NaOH?

**13**.

## What is the pH of a 1.9 10 ⁻ ³ M RBOH solution?

2 Answers By Expert Tutors

the [H^{1}^{+}] = 10^{–}^{14} / 1.9 x 10^{–}^{3} = 5.3 x 10^{–}^{12} . Take the negative log of this to get pH = **11.3**.

## What is the pH of a 0.0048 M KOH solution?

**16.32**| Chegg.com.

## What is the pH of a 0.050 M HBr solution?

## What is the pH of a 0.050 M HBr solution?

## Computing the pH value of 0.02 M HCl

## Calculate the pH of 0.2 M NaOH